Chem Final Review Packet
The full bag contains fewer molecules of each bag than it did at 0.0C
A plastic bag is weighed and then filled successively with two gases, X and Y. The following data are gathered: Temperature: 0.0C (273 K) Pressure: 1.00 atm Mass of empty bag: 20.77 g Mass of 1.12 liters of air at conditions given: 1.30 g Volume of bag: 1.12 liter Molar volume at STP: 22.4 liters The bag is emptied and refilled, successively, with gases X and Y, this time at 1 atm pressure and a temperature 30C higher. Assume that the volume of the bag is the same as before. Which one of the following statements is wrong? A) The full bag contains fewer molecules of each bag than it did at 0.0C B) The ratio of the density of gas Y to the density of gas X is the same at 0.0 C) The molar masses of the two gases are the same as they were at 0.0C D) The mass of each gas filling the bag is now 303/273 E) The average velocity of the molecules of gas X at 30C is higher than it was at 0.0C
0.00649
Express the number 6.49 x 10^-3 in common decimal form. A) 0.00649 B) 6.49 C) 6490 D) 0.0649 E) 0.000649
B2H6
A 1.00-g sample of a gaseous compound of boron and hydrogen occupies 0.820 L at 1.00 atm and 3C. What could be the molecular formula for the compound? A) BH3 B) B2H6 C) B4H10 D) B3H12 E) B5H14
0.260 atm
A 3.31-g sample of lead nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an evacuated cylinder with a volume of 2.37 L. The salt decomposes when heated, according to the equation: 2Pb(NO3)2(s) --> 2PbO(s) + 4NO2(g) + O2 (g) Assuming complete decomposition, what is the pressure in the cylinder after decomposition and cooling to a temperature of 300. K? Assume the PbO(s) takes up negligible volume. A) 0.260 atm B) 0.208 atm C) 0.0519 atm D) 0.364 atm E) 34.4 atm
C
A compound is composed of element X and hydrogen. Analysis shows the compound to be 80% X by mass, with three times as many hydrogen atoms as X atoms per molecule. Which element is element X? A) He B) C C) F D) S E) none of these
11.4 L
A fuel-air mixture is placed in a cylinder fitted with a piston. The original volume is 0.310-L. When the mixture is ignited, gases are produced and 935 J of energy is released. To what volume will the gases expand a constant pressure of 635 mmHg, if all the energy released is converted to work to push the piston? A) 10.7 L B) 8.02 L C) 11.4 L D) 11.0 L E) 1.78 L
2
A given sample of a xenon fluoride compound contains molecules of a single type XeFn, where n is some whole number. Given that 8.06 x 10^20 molecules of XeFn weigh 0.227 g, calculate n. A) 1 B) 6 C) 4 D) 3 E) 2
40%
A mixture of KCl and KNO3 is 44.20% potassium by mass. The percentage of KCl in the mixture is closest to A) 40% B) 50% C) 60% D) 70% E) 80%
1.42 liters
A sample of a gas occupies a volume of 2.62 liters at 25C and 1.00 atm. What will be the volume at 50.0C and 2.00 atm? A) 1.42 liters B) 2.62 liters C) 4.83 liters D) 5.68 liters E) 10.5 liters
homogeneous mixture
A solution is also called a A) homogeneous mixture B) heterogeneous mixture C) pure mixture D) compound E) distilled mixture
transition elements
An element with the electron configuration [Xe] 6s2 4f14 5d7 would belong to which class on the periodic table? A) transition elements B) alkaline earth elements C) rare earth elements D) none of the above
tend to gain electrons in chemical reactions
All of the following are characteristics of metals except: A) good conductors of heat B) malleable C) ductile D) often lustrous E) tend to gain electrons in chemical reactions
A, B, and C
Alpha particles beamed at thin metal foil may A) pass directly through without changing direction B) be slightly diverted by attraction to electrons C) be reflected by direct contact with nuclei D) A and C E) A, B, and C
6.4 kg NH3
Ammonia can be made by reaction of water with magnesium nitride as shown by the following unblanaced equation: Mg3N2(s) + H2O(l) --> Mg(OH)2(s) + NH3(g) If this process is 80% efficient, what mass of ammonia can be prepared from 19.0 kg magnesium nitride? A) 2.6 kg NH3 B) 6.4 kg NH3 C) 5.1 kg NH3 D) 3.2 kg NH3 E) 15 kg NH3
EF4
An element E has the electron configuration [Kr] 5s2 4d10 5p2. The formula for the fluoride of E is most likely A) EF14 B) EF4 C) EF D) EF6 E) EF8
all of these
An example of a pure substance is A) elements B) compounds C) pure water D) carbon dioxide E) all of these
A, B, and C
An isotope, X, of a particular element has an atomic number of 15 and a mass number of 31. Therefore: A) X is an isotope of phosphorus B) X has 16 neutrons per atom C) X has an atomic mass of 30.973 D) A and B E) A, B and C
No reaction will occur
Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statements is correct? A) Both KNO3 and NH4SO4 precipitate from solution B) A gas is released C) NH4SO4 will precipitate from solution D) KNO3 will precipitate from solution E) No reaction will occur
1.81 x 10^24 nitrogen atoms
Calculate the number of nitrogen atoms in 240. g of ammonium nitrate A) 2.01 x 10^23 nitrogen atoms B) 6.02 x 10^23 nitrogen atoms C) 1.20 x 10^24 nitrogen atoms D) 1.81 x 10^24 nitrogen atoms E) 3.61 x 10^24 nitrogen atoms
C(gr) + 1/2O2(g) --> CO(g), ^H= -110.5 kJ
Choose the correct equation for the standard enthalpy of formation of CO(g), where ^Hf for CO= -110.5 kJ/mol (gr indicates graphite) A) 2C(gr) + O2(g) --> 2CO(g), ^H= -110.5 kJ B) C(gr) + O(g) --> CO(g), ^H= -110.5 kJ C) C(gr) + 1/2O2(g) --> CO(g), ^H= -110.5 kJ D) C(gr) + CO2(g) --> 2CO(g), ^H= -110.5 kJ E) CO(g) --> C(gr) + O(g), ^H= -110.5 kJ
The mean square velocity of molecules in sample A is twice as large as the mean square velocity of molecules in sample B
Consider the following gas samples: Sample A Sample B Which of the following statements is false? A) The volume of sample A is twice the volume of Sample B B) The average kinetic energy of the molecules in sample A is twice the average kinetic energy of the molecules in sample B C) The fraction of molecules in sample A, having a kinetic energy greater than some high fixed value, is larger than the fraction of molecules in sample B, having kinetic energies greater than that same high fixed value D) The mean square velocity of molecules in sample A is twice as large as the mean square velocity of molecules in sample B E) Assuming identical inter molecular forces in the two samples, sample A should be more nearly ideal than sample B
n=4 to n=3
Consider the following portion of the energy-level diagram for hydrogen: n=4 -0.1361 x 10^-18 J n=3 -0.2420 x 10^-18 J n=2 -0.5445 x 10^-18 J n=1 -2.178 x 10^-18 J For which of the following transitions does the light emitted have the longest wavelength? A) n=4 to n=3 B) n=4 to n=2 C) n=4 to n=1 D) n=3 to n=2 E) n=2 to n=1
42.7 g
Consider the following reaction: Ch4(g) + 4Cl2(g) --> CCl4(g) + 4HCl(g) What mass of CCl4 will be formed if 1.20 moles of methane react with 1.11 moles of chlorine? A) 185 g B) 171 g C) 683 g D) 42.7 g E) 19.7 g
Lead
Consider the following specific heats of metals Metal Specific Heat If the same amount of heat is added to 25.0 g of each of the metals, which are all the same initial temperature, which metal will have the highest temperature? A) Zinc B) Magnesium C) Iron D) Silver E) Lead
17 lbs
Convert 7.9 kg to lb. (1 kg = 2.205 lb)
0.00028 mol
Diabetics often need injections of insulin to help maintain the proper blood glucose levels in their bodies. How many moles of insulin are needed to make up 45 mL of 0.0062 M insulin solution? A) 0.00056 mol B) 0.14 mol C) 7.3 mol D) 0.28 mol E) 0.00028 mol
Oxygen gas is limiting
Equal masses (in grams) of hydrogen gas and oxygen gas are reacted to form water. Which substance is limiting? A) Oxygen gas is limiting B) Hydrogen gas is limiting C) Water is limiting D) Nothing is limiting E) More information is needed to answer this question
0.353 J/g*C
Exactly 123.7 J will raise the temperature of 10.0 g of a metal from 25.0C to 60.0C. What is the specific heat capacity of the metal? A) 2.83 J/g*C B) 0.353 J/g*C C) 24.9 J/g*C D) 29.6 J/g*C E) none of these
None of the above is false
For a particular process q=-17 kJ and w= 21 kJ. Which of the following statements is false? A) Heat flows from the system to the surroundings B) The system does work on the surroundings C) E= +4 kJ D) The process is exothermic E) None of the above is false
$200
For spring break you and some friends plan a road trip to a sunny destination that is 2105 miles away. If you drive a car that gets 33 miles per gallon and gas costs $3.199/gal, about how much will it cost to get to your destination? A) $410 B) $220 C) $200 D) $660 E) $6700
29.1 g P4O10
For the reaction P4O10(s) + 6H2O(l) --> 4H3PO4(aq), what mass of P4O10 must be consumed if 3.71 x 10^23 molecules of H2O are also consumed? A) 1.05 x 10^3 g P4O10 B) 29.1 g P4O10 C) 175 g P4O10 D) 1.85 g P4O10 E) 66.6 g P4O10
Cl2
For which gas are the molecules diatomic? A) He B) Cl2 C) CH4 D) NH3 E) all gases the same
Ti
For which of the following elements does the electron configuration for the lowest energy state show a partially filled d orbital? A) Ti B) Rb C) Cu D) Ga E) Kr
deci= 10
For which pair is the SI prefix not matched correctly with its meaning? A) mega = 10^6 B) kilo = 1000 C) deci = 10 D) nano = 10^-9 E) centi = 0.01
Cl2
Four identical 1.0-L flasks contain the gases He, Cl2, CH4, and NH3, each at 0C and 1 atm pressure. Which gas has the highest density? A) He B) Cl2 C) CH4 D) NH3 E) all gases the same
1, 2, 1, 6
Give (in order) the correct coefficients to balance the following reaction: H2SnCl6 + H2S --> SnS2 + HCl A) 1, 2, 1, 6 B) 1, 2, 2, 2 C) 1, 1, 1, 6 D) 6, 2, 1, 1 E) 2, 4, 2 6
0.67
Given reaction N2 + 3H2 --> 2NH3, you mix 1 mol of each of nitrogen and hydrogen gases under the same conditions in a container fitted with a piston. Calculate the ratio of volumes of the container (Vf/Vi) A) 0.67 B) 1.00 C) 1.33 D) 1.50 E) none of these
-610.1 kJ
Given the heat of the following reactions: I. P4(s) + 6Cl2(g) --> 4PCl3(g) -1225.6 II. P4(s) + 5O2(g) --> P4O10(g) -2967.3 III. PCl3(s) + Cl2(g) --> PCl5(g) -84.2 IV. PCl3(g) + 1/2 O2(g) --> Cl3PO(g) -285.7 Calculate the value of ^H for the reaction below: P4O10(s) + 6PCl5(g) --> 10Cl3PO(g) A) -110.5 kJ B) -610.1 kJ C) -2682.2 kJ D) -7555.0 kJ E) None of these is within 5% of the correct answer
32
How many electrons can be contained in all of the orbitals with n=4? A) 2 B) 8 C) 10 D) 18 E) 32
10
How many electrons in an atom can have the quantum numbers n=3, l=2? A) 2 B) 5 C) 10 D) 18 E) 6
8.98 g
How many grams of potassium are in 27.8 g of K2CrO7? A) 4.49 g B) 1.422 g C) 8.98 g D) 78.2 g E) 55.6 g
2
How many of the following electron configurations for the species in their ground state are correct? I. Ca: 1s2 2s2 2p6 3s2 3p6 4s2 II. Mg: 1s2 2s2 2p6 3s1 III. V: [Ar] 3s2 3d3 IV. As: [Ar] 4s2 3d10 4p3 V. P: 1s2 2s2 2p6 3p5 A) 1 B) 2 C) 3 D) 4 E) 5
8
How many oxygen atoms are there in one formula unit of Ca3(PO4)2? A) 2 B) 4 C) 6 D) 8 E) none of these
34, 45, 36
How many protons, neutrons, and electrons, in that order are present in the anion formed by one atom of 79Se? A) 34, 34, 45 B) 34, 45, 34 C) 32, 45, 34 D) 34, 45, 36 E) 36, 45, 36
1230.
How should the number 1.230 x 10^3 be properly expressed as a decimal? A) 1230 B) 0.001230 C) 1230.0 D) 1230.
69.9%
Hydrocortisone valerate is an ingredient in hydrocortisone cream, prescribed for skin problems. Its molecular formula is C26H38O6. What is the percent by mass of carbon in hydrocortisone valerate? A) 69.9% B) 43.6% C) 54.2% D) 76.9% E) 60.1%
13.53%
If all the chloride in a 3.734-g sample of an unknown metal chloride is precipitated as AgCl with 70.90 mL of 0.2010 M AgNO3, what is the percentage of chloride in the sample? A) 50.52% B) 13.53% C) 1.425% D) 7.391% E) none of the above
The y, or vertical, intercept is the weight of the empty beaker
If volume of liquid is plotted along the horizontal axis, and total mass of beaker plus liquid is plotted on the vertical axis: A) The x, or horizontal, intercept is the negative value of the weight of the beaker B) The y, or vertical, intercept is the weight of the empty beaker C) The slope of the line is 1.0 D) The line will pass through the origin E) The slope of the line is independent of the identity of the liquid
The chemical reaction is absorbing energy
In the lab, you mix two solutions (each originally at the same temperature) and the temperature of the resulting solution decreases. Which of the following is true? A) The chemical reaction is releasing energy B) The energy released is equal to s x m x ^T C) The chemical reaction is absorbing energy D) The chemical reaction is exothermic E) More than one of these
I2
In which of the following does iodine have the lowest oxidation state? A) LiIO3 B) IO2 C) I2O D) NH4I E) I2
NO2
In which of the following does nitrogen have an oxidation state of +4? A) HNO3 B) NO2 C) N2O D) NH4Cl E) NaNO2
N2O
In which of the following does nitrogen have the lowest oxidation state? A) HNO3 B) NO2 C) N2O D) NH4Cl E) NaNO2
14
It l=3, how many electrons can be contained in all the possible orbitals? A) 7 B) 6 C) 14 D) 10 E) 5
70%
Naturally occurring copper exists in two isotopic forms: 63Cu and 65Cu. The atomic mass of copper is 63.55 amu. What is the approximate natural abundance of 63Cu? A) 63% B) 90% C) 70% D) 50% E) 30%
28.09 amu
Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.23% abundance), X-29 (28.976 amu, 4.67% abundance), and X-30 (29.974 amu, 3.10% abundance). Calculate the atomic weight of X. A) 28.09 amu B) 48.63 amu C) 27.63 amu D) 28.97 amu E) 86.93 amu
n=1, l=1, m1=0, ms= 1/2
Which of the following combinations of quantum numbers is not allowed? A) n=1, l=1, m1=0, ms= 1/2 B) n=3, l=0, m1=0, ms= -1/2 C) n=2, l=1, m1=-1, ms= 1/2 D) n=4, l=3, m1=-2, ms= -1/2 E) n=4, l=2, m1=0, ms= 1/2
2
Of energy, work, enthalpy, and heat, how many are state functions? A) 0 B) 1 C) 2 D) 3 E) 4
Ba
Of the following elements, which has the lowest first ionization energy? A) Ba B) Ca C) Si D) P E) Cl
P
Of the following elements, which needs three electrons to complete its valence shell? A) Ba B) Ca C) Si D) P E) Cl
H2
Of the following real gases, which would be expected to have the lowest van der Waals correction for inter molecular attractions? A) H2 B) Cl2 C) NH3 D) O2 E) not enough information to determine
176 g/mol
One molecule of a compound weights 2.93 x 10^-22 g. The molar mass of this compound is: A) 2.06 g/mol B) 567 g/mol C) 168 g/mol D) 176 g/mol E) none of these
F, Cl, S
Order the elements S, Cl, and F in terms of increasing ionization energy. A) S, Cl, F B) Cl, F, S C) F, S, Cl D) F, Cl, S E) S, F, Cl
H2SO4
Phosphoric acid can be prepared by reaction of sulfuric acid with "phosphate rock" according to the equation: Ca3(PO4)2 + 3H2SO4 --> 3CaSO4 + 2H3PO4 Suppose the reaction is carried out starting with 129 g of Ca3(PO4)2 and 97.4 g of H2SO4. Which substance is the limiting reactant? A) Ca3(PO4)2 B) H2SO4 C) CaSO4 D) H3PO4 E) none of these
[Ar] 4s1 3d10
Select the correct electron configuration for Cu. A) [Ar] 4s2 3d9 B) [Ar] 4s1 3d10 C) [Ar] 4s2 4p6 3d3 D) [Ar] 4s2 4d9 E) [Ar] 3d10
0.0876 M
Sulfamic acid, HSO3NH2 (molar mass =(7.1 g/mol), is a strong monoprotic acid that can be used to standardize a strong base: HSO3NH2(aq) + KOH(aq) --> KSO2NH2 (aq) + H2O(l) A 0.165-g sample of HSO2NH2 required 19.4 mL of an aqueous solution of KOH for a complete reaction. What is the molarity of the KOH solution? A) 0.00170 M B) 8.76 M C) 0.0876 M D) 0.0330 M E) none of these
1.52 x 10^6 g
Suppose that you purchased a water bed with the dimensions 2.55 m x 2.53 dm x 235 cm. What mass of water does this bed contain? A) 1.52 x 10^3 g B) 1.52 x 10^4 g C) 1.52 x 10^5 g D) 1.52 x 10^8 g E) 1.52 x 10^6 g
You must convert percent by mass to relative numbers of atoms
Suppose you are given the percent by mass of the elements in a compound and you wish to determine the empirical formula. Which of the following is true? A) You must convert percent by mass to relative numbers of atoms B) You must assume exactly 100.0 g of the compound C) You must divide all of the percent by mass numbers by the smallest percent by mass D) You cannot solve for the empirical formula without the molar mass E) At least two of the above (A-D) are true
1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d10 5p2
The complete electron configuration of tin is A) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5d10 5p2 B) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4d10 4p2 C) 1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d10 5d10 5p2 D) 1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d10 5p2 E) none of these
It will float on top
The density of gasoline is 0.7025 g/mL at 20C. When gasoline is added to water: A) It will float on top B) It will sink to the bottom C) It will mix so, you can't see it D) The mixture will improve the running of the motor E) None of these things will happen
2.1 x 10^4 m
The distance of 21 km equals A) 0.021 m B) 0.21 m C) 210 m D) 2100 m E) 2.1 x 10 ^4 m
75 protons, 110 neutrons
The element rhenium (Re) exists as two stable isotopes and 18 unstable isotopes. Rhenium-185 has in its nucleus A) 75 protons, 75 neutrons B) 75 protons, 130 neutrons C) 130 protons, 75 neutrons D) 75 protons, 110 neutrons E) not enough information
All of its hydrocarbon chains contain the same number of carbon atoms
The following statements concerning petroleum are all true except: A) It is a thick, dark liquid composed mostly of hydrocarbons B) It must be separated into fractions (by boiling) in order to be used efficiently C) Some of the commercial uses of petroleum fractions include gasoline and kerosene D) It was probably formed from the remains of ancient marine organisms E) All of its hydrocarbon chains contain the same number of carbon atoms
has the lowest ratio of moles available/ coefficients in the balance equation
The limiting reactant in a reaction A) has the lowest coefficient in a balanced equation B) is the reactant for which you have the fewest number of moles C) has the lowest ratio of moles available/ coefficients in the balance equation D) has the lowest ratio of coefficient in the balanced equation/ moles available E) none of these
none of the above
The limiting reactant in a reaction A) is the reactant for which there is the least amount in grams B) is the reactant which has the lowest coefficient in a balanced equation C) is the reactant for which there is the most amount in grams D) is the reactant for which there is the fewest number of moles E) none of the above
At 323F, the indium is partially solid and partially liquid; there is an equilibrium between the two states
The melting point of indium is 156.2C. At 323F, what is the physical state of indium? A) solid B) liquid C) gas D) not enough information E) at 323F, the indium is partially solid and partially liquid; there is an equilibrium between the two states
85.05%
The molar mass of an insecticide, dibromoethane, is 187.9 g/mol. Its molecular formula is C2H4Br2. What percent by mass of bromine does dibromoethane contain? A) 42.52% B) 2.14% C) 85.05% D) 12.78% E) 6.39%
3OH-(aq)
The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species? A) 3Al3+ (aq) B) OH- (aq) C) 3OH- (aq) D) 2Al3+ (aq) E) 2Al(OH)3(s)
3Ca2+ (aq)
The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species? A) 2Br- (aq) B) PO4^3- (aq) C) 2Ca3(PO4)2(s) D) 6NaBr(aq) E) 3Ca2+ (aq)
CO2
The rate of effusion of an unknown gas was measured and found to be 11.9 mL/min. Under identical conditions, the rate of effusion of pure oxygen (O2) gas is 14.0 mL/min. Based on this information, the identity of the unknown gas could be: A) F2 B) NO C) CO2 D) C2H2 E) none of these
2.52 atm
The valve between the 2.00-L bulb, in which the gas pressure is 1.80 atm, and the 3.00-L bulb, in which the gas pressure is 3.00 atm, is opened. What is the final pressure in the two bulbs, the temperature remaining constant? A) 0.720 atm B) 2.28 atm C) 2.52 atm D) 1.80 atm E) 2.40 atm
the finite volume of molecules
The van der Waals equation, nRT = [P +a(n/V^2](V-nb), incorporates corrections to the ideal gas law in order to account for the properties of real gases. One of the corrections account for law in order to account for the properties of real gases. One of the corrections accounts for A) the possibility of chemical reaction between molecules B) the finite volume of molecules C) the quantum behavior of molecules D) the fact that average kinetic is inversely proportional to temperature E) the possibility of phase changes when the temperature is decreased or the pressure is increased
Ne
Which of the following atoms has the largest ionization energy? A) O B) Li C) Ne D) Be E) K
4.22 x 10^-22 g
What is the mass of 4 atom(s) of copper in grams? A) 254.2 g B) 2.37 x 10^21 g C) 9.57 x 10^-24 g D) 6.022 x 10^23 g E) 4.22 x 10^-22 g
283 J/g*C
What is the specific heat capacity of a metal if it requires 178.1 J to change the temperature of 15.0 g of the metal from 25.00 C to 32.00 C A) 0.590 J/g*C B) 11.9 J/g*C C) 25.4 J/g*C D) 29.6 J/g*C E) 283 J/g*C
0.60 J/g*C
What is the specific heat capacity of silver if it requires 86.3 J to raise the temperature of 15 grams of silver by 25C? A) 4.3 J/g*C B) 0.23 J/g*C C) 0.14 J/g*C D) 0.60 J/g*C E) none of these
5.4 g
What mass of NaOH is required to react exactly with 25.0 mL of 2.7 M H2SO4? A) 2.7 g B) 0.7 g C) 5.4 g D) 135 g E) none of these
3, 3
When 87.7 is added to 73.841, the result should be reported with ___ significant figures. And when 87.7 is divided by 73.841 the result should be reported with ___ significant figures. A) 3, 3 B) 3, 5 C) 4, 3 D) 4, 4
none of these
When solutions of carbonic acid and copper(II) hydroxide react, which of the following are spectator ions? A) hydrogen ion B) carbonate ion C) copper(II) ion D) hydroxide ion E) none of these
hydrogen ion
When solutions of carbonic acid and potassium hydroxide react, which of the following are NOT present in the complete ionic equation? A) hydrogen ion B) carbonate ion C) potassium ion D) hydroxide ion E) water
CaCO3(s)
When solutions of cobalt(II) chloride and carbonic acid react, which of the following terms will be present in the net ionic equation? A) CoCO3(s) B) H+(aq) C) 2CoCO3(s) D) 2Cl-(aq) E) two of these
I, IV and II, V
Which among the following represent a set of isotopes? Atomic nuclei containing: I. 20 protons and 20 neutrons II. 21 protons and 19 neutrons III. 22 neutrons and 18 protons IV. 20 protons and 22 neutrons V. 21 protons and 20 neutrons A) I, II, III B) III, IV C) I, V D) I, IV, and II, V E) no isotopes are indicated
ultraviolet, visible, infrared
Which has these types of electromagnetic radiation arranged in order of decreasing energy? A) visible, ultraviolet, x-ray B) radiowaves, visible, ultraviolet C) ultraviolet, visible, infrared D) x-ray, visible, ultraviolet E) none of these
ultraviolet, visible, infrared
Which has these types of electromagnetic radiation arranged in order of decreasing frequency? A) visible, ultraviolet, x-ray B) radiowaves, visible, ultraviolet C) ultraviolet, visible, infrared D) x-ray, visible, ultraviolet E) none of these
transition metals
Which metals form cations with varying positive charges? A) transition metals B) Group 1 metals C) Group 2 metals D) Group 3 metals E) metalloids
Cesium, Ce
Which of the following are incorrectly paired? A) Copper, Cu B) Carbon, C C) Cobalt, Co D) Calcium, Ca E) Cesium, Ce
14/8 N
Which of the following atomic symbols is incorrect? A) 14/6 C B) 37/17 Cl C) 32/15 P D) 39/19 K E) 14/8 N
Mg(OH)2 is magnesium dihydroxide
Which of the following compounds is incorrectly named? A) Mg(OH)2 is magnesium dihydroxide B) CaO is calcium oxide C) NH4NO3 is ammonium nitrate D) K3PO4 is potassium phsphate E) MgSO3 is magnesium sulfite
That of Al is higher than that of Mg because electrons are taken from the same energy level, but the Al atom has one more proton
Which of the following concerning second ionization energies is true? A) That of Al is higher than that of Mg because Mg wants to lose the second electron, so it is easier to take the second electron away B) That of Al is higher than that of Mg because electrons are taken from the same energy level, but the Al atom has one more proton C) That of Al is lower than that of Mg because Mg wants to lose the second electron, thus the energy change is greater D) That of Al is lower than that of Mg because the second electron taken from Al is in a p orbital, thus it is easier to take E) The second ionization energies are equal for Al and Mg
4
Which of the following could not be a valid m1 quantum number for a 4d orbital? A) 2 B) 0 C) -2 D) 1 E) 4
Cr
Which of the following electron configurations is different from that expected? A) Ca B) Sc C) Ti D) V E) Cr
X(g) + e- => X+(g) +e-
Which of the following equations correctly represents the process involved in the electron affinity of X? A) X+(g) + e- => X(g) B) X+ (g) + Y-(g) => XY(g) C) X(g) + e- => X+(g) +e- D) X(g) => X+(g) + e- E) X+(g) => X+ (aq)
2KClO3 --> 2KCl + 3/2 O2
Which of the following equations is not balanced? A) 4Al + 3O2 --> 2Al2O3 B) C2H6 + 7/2 O2 --> 2CO2 + 3H2O C) 2KClO3 --> 2KCl + 3/2 O2 D) 4P4 + 5S8 --> 4P4S10 E) P4 + 5O2 --> P4O10
4.12 x 10^5 s-1
Which of the following frequencies corresponds to light with the longest wavelength? A) 3.00 x 10^13 s-1 B) 4.12 x 10^5 s-1 C) 8.50 x 10^20 s-1 D) 9.12 x 10^12 s-1 E) 3.20 x 10^9 s-1
two of the above
Which of the following have 10 electrons in the d orbitals? A) Mn B) Fe C) Cu D) Zn E) two of the above
NH4+
Which of the following ions forms the fewest insoluble salts? A) Al3+ B) Cl C) NH4+ D) OH- E) Mg2+
Ca2+
Which of the following ions is most likely to form an insoluble sulfate? A) K+ B) Li+ C) Ca2+ D) S2- E) Cl-
HClO4
Which of the following is a strong acid? A) HF B) KOH C) HClO4 D) HClO E) HBrO
methane
Which of the following is both a greenhouse gas and a fuel? A) carbon dioxide B) coal C) freon D) methane E) nitrogen
All collisions between molecules are elastic
Which of the following is included as a postulate in the kinetic molecular theory of an ideal gas? A) The distance between gas molecules is small compared with the size of the molecule B) All collisions between molecules are elastic C) In an average collision between molecules, both molecules have the same kinetic energy D) All molecules move randomly in zigzag directions E) All the molecules have the same velocity
gram
Which of the following is not a fundamental metric unit? A) meter B) second C) gram D) mole
liter
Which of the following is not a fundamental metric unit? A) meter B) second C) kilogram D) liter
The average velocity of the gas particles is directly proportional to the absolute temperature
Which of the following is not an assumption of the kinetic molecular theory for a gas? A) Gases are made up of tiny particles in constant chaotic motion B) Gas particles are very small compared to the average distance between the particles C) Gas particles collide with the walls of their container in elastic collisions D) The average velocity of the gas particles is directly proportional to the absolute temperature E) All of the above are assumptions of the kinetic molecular theory
HNO3- weak acid
Which of the following is paired incorrectly? A) H2SO4- strong acid B) HNO3- weak acid C) Ba(OH)2- strong base D) HCl- strong acid E) NH3- weak base
\
Which of the following is the best qualitative graph of P versus molar mass of a 1-g sample of different gases at constant volume and temperature? A) / B) / (starts higher) C) ---- D) \ E) none of these
All of these are equally probable
Which of the following is the least probable concerning five measurements taken in the lab? A) The measurements are accurate and precise B) The measurements are accurate but not precise C) The measurements are precise but not accurate D) The measurements are neither accurate nor precise E) All of these are equally probable
all
Which of the following name(s) is(are) correct? 1. sulfide, S^-2 2. ammonium chloride, NH4Cl 3. acetic acid, HC2H3O2 4. barium oxide, BaO A) all B) none C) 1, 2 D) 3, 4 E) 1, 3, 4
SO and SO2
Which of the following pairs can be used to illustrate the law of multiple proportions? A) SO and SO2 B) CO and CaCO3 C) H2O and C12H22O11 D) H2SO4 and H2S E) KCl and KClO2
BaPO4, barium phosphate
Which of the following pairs is incorrect? A) NH4Br, ammonium bromide B) K2CO3, potassium carbonate C) BaPO4, barium phosphate D) CuCl, copper(I) chloride E) MnO2, manganese(IV) oxide
phosphorous pentoxide, P2O5
Which of the following pairs is incorrect? A) iodine trichloride, ICl3 B) phosphorous pentoxide, P2O5 C) ammonia, NH3 D) sulfur hexafluoride, SF6 E) all of the above pairs are correct
O3
Which of the following pollutant gases is not produced directly in a combustion engine? A) CO B) CO2 C) O3 D) NO E) NO2
Br(g) ---> Br+(g) +e-
Which of the following processes represents the ionization energy of bromine? A) Br(s) ---> Br+(g) +e- B) Br(l) ---> Br+(g) +e- C) Br(g) ---> Br+(g) +e- D) Br(s) ---> Br+(s) +e- E) Br2(g) ---> Br2+(g) +e-
Real gases consist of molecules or atoms that have volume
Which of the following properties of a real gas is related to the b coefficient in the van der Waals equation? A) Real gases consist of molecules or atoms that have volume B) The average speed of the molecules of a real gas increases with temperature C) These are attractive forces between atoms or molecules of a real gas D) The rate of effusion of a gas is inversely proportional to the square root of the molecular weight of the gas E) None of these
All of these are soluble in water
Which of the following salts is insoluble in water? A) Na2S B) K2CO3 C) Pb(NO3)2 D) CaCl2 E) All of these are soluble in water
All of the above statements (A-D) are true
Which of the following statements about atomic structure is false? A) An atom is mostly empty space B) Almost all of the mass of the atom is concentrated in the nucleus C) The protons and neutrons in the nucleus are very tightly packed D) The number of protons and neutrons is always the same in the neutral atom E) All of the above statements (A-D) are true
When filling orbitals of equal energy, two electrons will occupy the same orbital before filling a new orbital
Which of the following statements about quantum theory is incorrect? A) The energy and position of an electron cannot be determined simultaneously B) Lower energy orbitals are filled with electrons before higher energy orbitals C) When filling orbitals of equal energy, two electrons will occupy the same orbital before filling a new orbital D) No two electrons can have the same four quantum numbers E) All of these are correct
I, II, IV
Which of the following statements are true of unanium-238? I. Its chemical properties will be exactly like those of uranium-235 II. Its mass will be slightly different from that of an atom of uranium-235 III. It will contain a different number of protons than an atom of uranium-235 IV. It is more plentiful in nature than uranium- 235 A) III, IV B) I, II, III C) I, II, IV D) II, III, IV E) all of these
Scientists believe that solids are mostly open space
Which of the following statements are true? A) Ions are formed by adding or removing protons or electrons B) Scientists believe that solids are mostly open space C) Heating water with a Bunsen burner results in a 2:1 mixture of hydrogen and oxygen gases D) At least two of the above statements (A-C) are true E) All of the statements (A-C) are false
It is impossible to accurately know both the exact location and momentum of a particle
Which of the following statements best describes the Heisenberg uncertainty principle? A) The exact position of an electron is always uncertain B) The velocity of a particle can only be estimated C) It is impossible to accurately know both the exact location and momentum of a particle D) The location and momentum of a macroscopic object are not known with certainty E) The location and momentum of a particle can be determined accurately, but not the identity of the particle
A and C
Which of the following statements is (are) true? A)18/8 O and 19/9 F have the same number of neutrons B) 14/6 C and 14/7 N are isotopes of each other because their mass numbers are the same C) 18/8 O^-2 has the same number of electrons as 20/10 Ne D) A and B E) A and C
If we have more mass of C2H6, then O2 must be limiting
Which of the following statements is always true concerning a reaction represented by the following balanced chemical equations? 2C2H6(g) + 7O2(g) --> 6H2O(l) + 4CO2(g) A) If we have equal masses of C2H6 and O2, there is no limiting reactant B) It we have an equal number of moles of C2H6 and O2, there is no limiting reactant C) If we have more mass of C2H6, then O2 must be limiting D) If we have more mass of O2, then C2H6 must be limiting E) none of these statements are true
The system does work on the surroundings when an ideal gas expands against a constant external pressure
Which of the following statements is correct? A) The internal energy of a system increases when more work is done by the system than heat was flowing into the system B) The internal energy of a system decreases when work is done on the system and heat is flowing into the system C) The system does work on the surroundings when an ideal gas expands against a constant external pressure D) All statements are true E) All statements are false
An orbital can accommodate at most two electrons
Which of the following statements is false? A) An orbital can accommodate at most two electrons B) The electron density at a point is proportional to u2 at that point C) The spin quantum number of an electron must be either 1/2 or -1/2 D) A 2p orbital is more penetrating than a 2s; i.e., it has a higher electron density near the nucleus and inside the charge cloud of a 1s orbital E) In the usual order of fillinf, the 6s orbital is filled before the 4f orbital
The volume of the sample would be zero at -273C
Which of the following statements is least likely to be true of a sample of nitrogen gas? A) Molecules of gaseous nitrogen are in constant random motion B) The pressure exerted by gaseous nitrogen is proportional to the absolute temperature of the gas C) The average kinetic energy of the gaseous nitrogen is proportional to the absolute temperature of the gas D) Collisions between the gaseous molecules are elastic E) The volume of the sample would be zero at -273C
The gas molecules have a very low molar mass
Which of the following statements is least likely to be true of a sample of nitrogen gas? A) The gas molecules are large enough to occupy a substantial amount of space B) A large number of molecules have speeds greater than the average speed C) The gas molecules have a very low molar mass D) The gas molecules attract one another E) None of these
It will be equal to and opposite in sign to the electron affinity of Mg2+
Which of the following statements is true about the ionization energy of Mg+? A) It will be equal to the ionization energy of Li B) It will be equal to and opposite to the electron affinity of Mg C) It will be equal to and opposite to the electron affinity of Mg+ D) It will be equal to and opposite to the electron affinity of Mg2+ E) None of the above
The krypton 1s orbital is smaller than the helium 1s orbital because krypton's nuclear charge draws the electrons closer
Which of the following statements is true? A) The krypton 1s orbital is smaller than the helium 1s orbital because krypton's nuclear charge draws the electrons closer B) The krypton 1s orbital is larger than the helium 1s orbital because krypton contains more electrons C) The krypton 1s orbital is smaller than the helium 1s orbital because krypton's p and d orbitals crowd the s orbitals D) The krypton 1s orbital and helium 1s orbital are the same size because both s orbitals can only have two electrons E) The krypton 1s orbital is larger than the helium 1s orbital because krypton's ionization energy is lower, so it's easier to remove electrons
1 microliter/ 1000 nL
Which of the following unit factors is incorrect? A) 1 microliter/ 1000 nL B) 1 cg/ 100 g C) 1 L/ 1000 mL D) 1000 m/ 1 km
CH4
Which of the following would have a higher rate of effusion than C2H2? A) N2 B) O2 C) Cl2 D) CH4 E) CO2
11.4 psi
Which of the following would represent the greatest pressure? A) 0.680 atm B) 517 mmHg C) 11.4 psi D) 62106 Pa E) 14.1 in Hg
The 5 lead by mass in the compound galena is the same for all pure samples obtained from any source
Which of these statements is a consequence (follows from) the Law of Multiple Proportions? A) All samples of chlorine contain 35Cl and 37Cl in the same (definite) ratio B) The mass of oxygen that is combined with a fixed mass of nitrogen in each of the binary nitrogen oxides can be expressed as a ratio of small whole numbers C) The atomic masses of all of the elements in the periodic table have fixed values D) The 5 lead by mass in the compound galena is the same for all pure samples obtained from any source E) None of these is correct
Mg2+, SO4^2-
Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed? A) Al3+, S2- B) Pb2+, Cl- C) Ba2+, PO2^3- D) Pb^2+, OH- E) Mg2+, SO4^2-
An atom of 18O has an equal number of protons and neutrons
Which statement is INCORRECT? A) An atom of 60ZN has an equal number of protons and neutrons B) An atom of 50Mn has an equal number of protons and neutrons C) An atom of 18O has an equal number of protons and neutrons D) An atom of 41K has an equal number of protons and neutrons E) An atom of 238U contains 146 neutrons
There are only three types of radioactivity known to scientists today
Which statement is not correct? A) The mass of an alpha particle is 7300 times that of the electron B) An alpha particle has a 2+ charge C) Three types of radioactivity emission are gamma rays, beta rays, and alpha particles D) A gamma ray is high energy light E) There are only three types of radioactivity known to scientists today
The amount of heat released in the process will depend on the path taken
Which statement is true of a process in which one mole of a gas is expanded from state A to state B? A) When the gas expands from state A to state B, the surroundings are doing work on the system B) The amount of work done in the process must be the same, regardless of the path C) It is not possible to have more than one path for a change of state D) The final volume of the gas will depend on the path taken E) The amount of heat released in the process will depend on the path taken
all have the same volume
You are holding four identical balloons each containing 10.0 g of a different gas. The balloon containing which gas is the largest balloon? A) H2 B) He C) Ne D) O2 E) All have the same volume
0.538 M
You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 1.72 M solution of AgNO3(aq). Calculate the concentration of Ag+ after the two solutions are mixed together. A) 0.00 M B) 0.538 M C) 1.08 M D) 0.088 M E) 0.215 M
3.50 M
You have two solutions of sodium chloride. One is a 2.00 M solution, the other is a 4.00 M solution. You have more of the 4.00 M solution and you add the solutions together. Which of the following could be the concentration of the final solution? A) 2.70 M B) 3.00 M C) 3.50 M D) 6.00 M E) 8.10 M
All are true
You mix 275.0 mL of 1.20 M lead(II)nitrate with 300.0 mL of 1.85 M potassium iodide. The lead(II) iodide is insoluble. Which of the following is false? A) The final concentration of Pb2+ ions is 0.0913 M B) You form 128 g of lead(II) iodide C) The final concentration of K+ is 0.965 M D) The final concentration of NO3- is 0.965 M E) All are true
0.056 mol
Zinc metal is added to hydrochloric acid to generate hydrogen gas, which is collected over a liquid whose vapor pressure is the same as pure water at 20.0C (18 torr). the volume of the gas mixture is 1.7 L and its total pressure is 0.810 atm Determine the number of moles of hydrogen gas present in the sample A) 42 mol B) 0.82 mol C) 1.3 mol D) 0.056 mol E) 22 mol
none of these
wPCl5 + xH2O --> yPOCl3 + zHCl The above equation if properly balanced when: A) w= 1, x=2, y=2, z=4 B) w= 2, x=2, y=2, z=2 C) w= 2, x=2, y=2, z=1 D) w= 1, x=1, y=1, z=2 E) none of these