Chem final
A hydrocarbon has the formula C5H12. What is the percent by mass of carbon in the compound? A. 83.2% B. 41.6% C. 16.8 %
A. 83.2%
Choose the pair of compounds with the same empirical formula. A. C2H2 and C6H6 B. NaHCO3 and NaCO3 C. K2CrO4 and Na2CO3
A. C2H2 and C6H6
Calculate the molecular formula of a compound with the empirical formula CH2O and a molar mass of 180g/mol A. C6H12O6 B. C5H10O5 C. C7H14O7
A. C6H12O6
A compound contains 40% carbon, 6.7% hydrogen ,and 53.3% oxygen (by mass). Calculate the empirical formula. A. CH2O B.C2H2O C. CH4O
A. CH2O
The form of EMR that has more energy per photon than ultraviolet rays but less energy per photon than gramma rays is A. Microwaves B. radio waves C. x rays
C. x rays
Determine the percentage composition (by mass) of oxygen in Li2SO4 A. 58.21% B. 14.55% C. 29.09%
A. 58.21%
1.2 moles of oxygen atoms represent A. 0.7x10^24 atoms B. 0.4 atoms C. 1.0x10^2 atoms
A. 0.7x10^24 atoms
Which represent the greatest mass A. 1.0 mol Rb B. 1.0 mol Fe C. all the same D. 1.0 mol Ti
A. 1.0 mol Rb
How many molecules of O2 are there in 2.2 moles of O2? A. 1.3x10^24 B. 3.7x10^24 C. 70 D. 14.55
A. 1.3x10^24
The molar mass of ammonium phosphate, (NH4)3 PO4 is A. 149.09 g/mol B. 113.01 g/mol C. 302.95 g/mol D. 165.09 g/mol
A. 149.09 g/mol
What is the molar mass of Ba(OH)2? A. 171.35 g/mol B. 291.67 g/mol C. 308.68 g/mol D. 154.34 g/mol
A. 171.35 g/mol
A 36.6 mol sample of Co represents how many atoms? A. 2.20x10^25 atoms B. 6.08x10^-23 atoms C. 1.65x10^22 atoms D. 1.30x10^27
A. 2.20x10^25 atoms
Convert 4.13 mol PCl5 to molecules A. 2.49x10^24 B. 6.86x10^24 C. 1.46x10^23
A. 2.49x10^24
8.52g of water contains how many molecules of water? A. 2.85x10^23 B. 7.07x10^22 C. 1.27x10^24
A. 2.85x10^23
Calculate the percentage composition (by mass) of Mg in Mg3 (AsO4)2 A. 20.8% B. 34.4% C. 36.3%
A. 20.8%
what is the mass of 1.819 mol of potassium sulfide? A. 200.6 g B. 187.8g C. 60.62g D. 129.4g
A. 200.6 g
What is the molar mass of nitroglycerin, C3H5(NO3)3? A. 227 g/mol B. 179 g/mol C. 199 g/mol
A. 227 g/mol
The molar mass of barium nitrate, Ba(NO3)2 is A. 261.35 g/mol B. 336.67 g/mol C. 293.35 g/mol
A. 261.35 g/mol
The molar mass of calcium phosphate, Ca(PO4)2 is A. 310.18 g.mol B. 365.07 g/mol C. 230.02 g/mol
A. 310.18 g.mol
The mass percent of chlorine in BaCl2 is A. 34% B. 17% C. 20.5%
A. 34%
The mass percent of hydrogen in NH4Br A. 4.12% B. 1.03% C. 5% D. 16.5%
A. 4.12%
What is the percentage (by mass) of carbon in glucose, C6H12O6 A. 40% B. 53.3% C. 25% D. 6.7%
A. 40%
Determine the percentage composition (by mass) of nitrogen in NH4NO2 A. 43.72% B. 21.86% C. 93.69% D. 25%
A. 43.72%
The form of EMR that has less energy per photon than infrared rays but more energy per photon than radio waves is A. microwaves B. ultraviolet C. grammas rays
A. microwaves
Which color of visible light has the most energy per photon A. violet B. blue C. green D. yellow
A. violet
The molar mass of blood sugar, C6H12O6, also known as glucose and dextrose, is A.180.16g/mol B. 6.02x10^23 g/mol C. 108.10g/mol D.168.06g/mol
A.180.16g/mol
A 3.37mol sample of aluminum represents how many atoms? A.2.03x10^24 atoms B. 5.60x10^24 atoms C. 1.25x10^23 atoms
A.2.03x10^24 atoms
A 1.50 mol sample of Zr represents how many atoms? A.9.03x10^23 atoms B. 2.49x10^24 atoms C. 4.01x10^23 atoms
A.9.03x10^23 atoms
the mass in grams of 3.5mol of nitrogen gas (N2) is A. none of these B. 49.3 g/mol C. 98.6 g.mol D. 6.02x10^23 g/mol
C. 98.6 g.mol
The rusting of iron is represented by the equation 4Fe+3O2 --> 2Fe2O3. If you have a 1.45mol sample of iron, how many moles of Fe2O3 will there be after the iron has rusted completely? A. 0.483mol B. 0.725mol C. 0.97mol
B. 0.725mol
For the reaction 2S+3O--> 2So3, how many mol of SO3 will be produced from 2.2mol O2 and excess S? A. 3.3mol B. 1.5mol C. 2.2mol
B. 1.5mol
A sample of metal weighing 2.51 g is combined with oxygen; the metal oxide weighs 3.01 g. The mass percent of oxygen in the compound is A. 86% B. 14% C. 19% D. 31.2%
B. 14%
What mass of carbon dioxide will be produced when 29.9g of butane reacts with am excess of oxygen in the following reaction? 2C4H10+ 13O2--> 8CO2+10H2O A. 181.1g B. 90.6g C. 11.32g
B. 90.6g
calculate the mass of 23.7 moles of He A. 6.02x10^23 B. 94.9 C. 5.92 D. 1.43x10^25
B. 94.9
Acetylene gas is 92.3% carbon and 7.7% hydrogen (by mass), and its molar mass is 26 g/mol. What is its molecular formula? A. CH B. C2H2 C. CH4 D. C4H4
B. C2H2
The balanced equation 2Cu+O2 --> 2CuO tells us that 4.0mol of Cu A. reacts with 4.0mol of O2 B. Produces 4mol of CuO C. Must react with 128g of O2
B. Produces 4mol of CuO
The balanced equation 2Cu+O2 --> 2CuO tells us that 4mol of Cu A. reacts with 4mol of O2 B. produces 4mol of CuO C. must react with 128g of O2
B. produces 4mol of CuO
The energy levels of the hydrogen atom (and all atoms) are ____, meaning that only certain discrete energy levels are allowed. A. varied B. quantized C. ramp-like
B. quantized
How many mol of oxygen are produced by decomposing 28.5g of H2O2 (molar mass 34g/mol) according to the equation: 2H2O2--> 2H2O+O2 A. 0.838mol B. 485mol C. 0.419mol D. 1.68mol
C. 0.419mol
In the reaction N2+3H2 --> 2NH3, how many moles of ammonia would be produced from 1.21mol of hydrogen and excess nitrogen? A. 1.57mol B. 3.63mol C. 0.807mol
C. 0.807mol
Calculate the mass of 3.64x10^19 molecules of HCl A. 6.04x10^5 g B. 1.66x10^6 g C. 2.20x10^-3 g D. 2.19x10^43 g
C. 2.20x10^-3 g
Refer to the following equation: 4NH3+7O2--> 4NO2+6H2O, how many molecules of NO2 are produced when 5.38mol of ammonia is completely reacted? A. 21.52 B. 6.48x10^24 C. 3.24x10^24
C. 3.24x10^24
When 3.4mol of Fe reacts with Cl2 according to the equation: 2Fe+3Cl2--> 2FeCl3 How many moles of Cl2 are required to react with all of the iron? A. 2.3mol B. 3.4mol C. 5.1mol D. 0.9mol
C. 5.1mol
An excess of Al and 7.9mol of Br2 are reacted according to the equation 2Al+3Br2--> 2ALBr3, how many moles of AlBr3 will be formed assuming 100% yield? A. 2.6mol B. 4mol C. 5.3mol
C. 5.3mol
Calculate the mass of 3.53x10^26 atoms of silver A. 5.86x10^2 g B. none of these C. 6.32x10^4 g D. 1.97x10^48 g
C. 6.32x10^4 g
Refer to the following equation: 4NH3+7O2--> 4No2+6H2O How many moles of ammonia will be required to produce 11.9 mol of water? A. 4.76mol B. 11.9mol C. 7.93mol D. 5.95mol
C. 7.93mol
For the equation C2H4+ 3O2--> 2CO2+2H2O If 5.5mol of CO2 are produced, how many moles of O2 were reacted? A. 3.6mol B. 6.8mol C. 8.2mol
C. 8.2mol
In the reaction 3Cl2+6NaOH--> 5NaCl+NaClO3+3H2O, how many moles of chlorine molecules are needed to react with 13.3g of NaOH? A. 1mol B. 0.333mol C. 0.67mol D. 0.166mol
D. 0.166mol
Calculate the number of molecules of Ch4 in 41g CH4 A. 2.5x10^25 molecules B. 4.0x10^26 molecules C. 1.1x10^21 molecules D. 1.5x10^24 molecules
D. 1.5x10^24 molecules
convert 92.1g Co to molecules A. 5.55x10^25 B. 2.58x10^3 C. 1.53x10^23 D. 1.98x10^24
D. 1.98x10^24
calculate the number of moles of Cl2 molecules in a sample that contains 7.380x10^25 molecules of Cl2. A. 4.444x10^49 mol B. 8.160x10^3 mol C. 2.451x10^2 mol D. 122.6mol
D. 122.6mol
Fe3O4 reacts with CO according to the equation Fe3O4+4CO--> 4CO2+3Fe, if 335.2g Fe2O4 is reacted with excess Co, what mass of CO2 will be produced? A. 63.71g B. 191.1g C. 127.42g D. 254.8g
D. 254.8g
6.13 moles of oxygen molecules contain how many oxygen atoms? A. 7.38x10^24 B. 98 C. 196 D. 3.69x10^24
D. 3.69x10^24
One mole of something consists of _____ units of that substance. A. 12.01 B. 1,008 C. 1.66x10^24 D. 6.022x10^23
D. 6.022x10^23
How many atoms are there in 71.9g of nickel? A. 4.33x10^25 B. none of these C. 1.23 D. 7.38x10^23
D. 7.38x10^23
4.04 mol of water weighs A. 78.5g B. 4.46g C. 2.24x10^-1 g D. 72.8g
D. 72.8g
A gaseous compound containing carbon and hydrogen was analyzed and found to consist of 83.65% carbon by mass. The molar mass of the compound is 86.2g/mol. What is molecular formula of the compound? A. C3H7 B. Ch2 C. C2H4 D. C6H14
D. C6H14
Calculate the mass, in grams, of 1.83x10^26 formula units of sulfur dioxide. A. 1.17x10^28g B. none of these C. 3.04x10^2g D. 4.74x10^0g E. 1.95x10^-4g
E. 1.95x10^-4g
how many mol of Ca atoms are in 613.3g Ca? A. 613.3mol B. 30.60 mol C. 6.535x10^2 mol D. 2.458x10^4 mol E. 15.30 mol
E. 15.30 mol
26.4g of Ni represents how many atoms? A. 0.450 atoms B. 1.59x10^25 atoms C. 4.38x10^-23 atoms D. 2.57x10^21 atoms E. 2.71x10^23 atoms
E. 2.71x10^23 atoms
A 3.1mol sample of KClO3 was decomposed according to the equation 2KClO3 --> 2KClO + 3O2 How many moles of O2 are formed assuming 100% yield? A. 2.1mol B. 2.6mol C. 3.1mol D. 1.6mol E. 4.7mol
E. 4.7mol
A 3.1mol sample of KClO3 was decomposed according to the equation 2KClO3--> 2KCl+3O2, how many moles of O2 are formed assuming 100% yield? A. 2.1mol B. 2.6mol C. 3.1mol D. 1.6mol E. 4.7mol
E. 4.7mol
How many atoms of calcium are present in 58.2g of calcium? A. none of these B. 6.02x10^23 C.2.41x10^24 D. 3.50x10^25 E. 8.74x10^23
E. 8.74x10^23
a gaseous compound containing carbon and hydrogen was analyzed and found to consist of 83.65% carbon by mass. What is the empirical formula of the compound? A. Ch2 B. CH3 C. C7H16 D. CH E. C3H7
E. C3H7
the empirical formula for the compound having the formula H2C2O4 is A. COH B. COH2 C. C2H2 D. C2O4H2 E. CO2H
E. CO2H
Which color of visible light has the least amount of energy per photon A. violet B. blue C. green D.yellow E. red
E. red
the amount of energy needed to heat 2.00g mercury from 50C to 85C is 9.87J. The specific heat capacity of this sample of mercury is a. 0.141 J/gC b. 0.058 J/gC c. 0.282 J/gC d. 345 J/gC
a. 0.141 J/gC
A 4.60g sample of iron is heated from 47C to 75C. The amount of energy required is 57.96J. The specific heat capacity of this sample of iron is a. 0.450 J/gC b. 1.233 J/gC c. 2.07 J/gC d/ 1623 J/gC
a. 0.450 J/gC
the electron configuration for the sulfur atom is a. 1s^2 2s^2 2p^6 3s^2 3p^4 b. 1s^2 2s^2 2p^6 3s^2 3p^6 c. 1s^2 2s^2 2p^6 3s^2 3p^2
a. 1s^2 2s^2 2p^6 3s^2 3p^4
the correct electron configuration for Ti is a. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2 b. 1s^2 2s^2 2p^6 3s^2 3p^6 3d^4 c. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3
a. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2
Which of the following is incorrect a. 2f b. 1s c. 5f d. 6p
a. 2f
How many lone pairs of electrons are there in the Lewis structure for compound HF a. 3 b. 4 c. 0
a. 3
a phosphorous atom needs to gain ___ electrons to achieve a noble gas configuration a. 3 b. 2 c. 4 d. 5
a. 3
how many joules of energy would be required to heat 15.9g of carbon from 23.6C to 54.2C? (Specific heat of carbon= .71J/gC) a. 3.5x10^2 b. 8.9x10^2 c. 6.1x10^2
a. 3.5x10^2
the number of polar covalent bonds is SF4 id a. 4 b. 3 c.1 d.2
a. 4
perform the indicated conversion 1.345kcal to J a. 5.627x10^3 b. 5.627 c. 5.627x10^-3
a. 5.627x10^3
a 6.75g sample of gold (specific heat capacity = 0.130J/gC) is heated using 55.8J of energy. If the original temperature of the gold is 25C, whats its final temp? a. 88.6C b. 38.6C c. 76.9C
a. 88.6C
perform the following conversion of pressure units 1.178 atm to torr a. 895.3 b. 645.2 c. 1.550x10^-3 d. 17.32
a. 895.3
which of the following has the nonpolar bonds a. Cl2 b. H2S c. OF2
a. Cl2
which elements has the fewest electrons in its valence shell a. Cs b. Mg c. P d. O
a. Cs
Which one of the following is ranked in order of largest to smallest atomic radius a. Cs>Mn>Ge>S>O b. Mn>Cs>O>S>Ge c. O>S>Ge>Mn>Cs
a. Cs>Mn>Ge>S>O
which of the following has the highest ionization energy a. F b. Be c. N d. C
a. F
All these atoms have seven electrons in their outermost energy levels except a. H b. F c. Cl d. Br
a. H
the most electronegative element of those listed is a. O b. Se c. Po
a. O
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3 is the electron configuration for which of the atoms a. V b. Ca c. Ar d. Sc
a. V
You have partially filled party ballon with 2.00g of helium gas. You then add 3.00g of hydrogen gas to the ballon. Assuming constant temp and pressure, how many times bigger is the party ballon-- comparing before and after the hydrogen gas has been added. Choose the best formula to use to solve this problem. (V= volumes of gas, n= moles, m= mass, p= pressure) a. V2/V1= n2/n1 b. V2/V1= m2/m1 c. P2/P1= n2/n1
a. V2/V1= n2/n1
which of the following is a valid unit for specific heat? (or specific heat capacity)? a. cal/gC b. cal c. cal/g d. C
a. cal/gC
___ is a flow of energy due to a temperature difference a. heat b. radiation c. matter d. gravity
a. heat
As the principal energy level increases in an atom's orbitals, the average distance of an electron energy level from the nucleus _____. a. increases b. decreases c. stays the same d. varies
a. increases
___ is a form of oxygen that protects us from high-energy radiation emitted by the sun a. ozone b. carbon dioxide c. ultraviolet
a. ozone
the group 3A elements thru the group 8A elements form an area of the periodic table where the electron sublevels being filled are a. p orbitals b. s and p orbitals c. d orbitals
a. p orbitals
When moving down a group (family) in the periodic table, the number of valence electrons a. remains constant b.. increases by 2 then 8 then 18 then 31 c. doubles with each move
a. remains constant
Which color of visible light has the shortest wavelength? a. violet b. red c. orange d.blue
a. violet
the specific heat capacity of gold is 0.13J/gC. How many calories of energy are needed to warm 0.570g of gold from 30C to 39.5C a. 0.70 cal b. 0.17 cal c. 1.2 cal d. 2.9cal
b. 0.17 cal
the specific heat capacity of silver is 0.24J/gC. How many J of energy are needed to warm 0.960g of silver from 25C to 27.5C a. 6.3J b. 0.58J c. 12.1J
b. 0.58J
A d sublevel can hold a maximum of a. 5 electrons b. 10 electrons c. 14 electrons
b. 10 electrons
the maximum electron capacity of an f sublevel is a. 18 b. 14 c. 10
b. 14
assume that 491.8 J of heat is added to 5g of water originally at 23C. what would be the final temperature of the water? (specific heat capacity of water= 4.184 J/gC) a. 23.5C b. 61.5C c. 74.5C d. 46.5C
b. 61.5C
perform the indicated conversion 38.86kJ to kcal a. 1.626x10^2 kcal b. 9.288 kcal c. 9.288x10^3 kcal
b. 9.288 kcal
which of the following compounds contains an ionic bond a. HCl b. NaCl c. CCl4
b. NaCl
which one of the following atoms has the partly filled d sublevel a. Ca b. Ni c. Zn d. As
b. Ni
which of the following processes is endothermic (into the system) a. water droplets condensing on a soda can of a hot summer day b. an ice pack getting cold (due to ammonium nitrate dissolving in water inside the pack) c. thermite reaction between iron oxide and aluminum
b. an ice pack getting cold (due to ammonium nitrate dissolving in water inside the pack)
if temperature and pressure are held constant, the volume and number of moles of a gas are a. independent of each other b. directly proportional c. inversely proportional d. equal
b. directly proportional
____ is a measure of the random motions of the components of a substance a. heat b. temperature c. energy d. radiation
b. temperature
Is a phenomenon that may be caused by the burning of fossil fuels, which increases the CO2 content in the earth's atmosphere a. acid rain b. the greenhouse effect c. infrared radiation
b. the greenhouse effect
Perform the following conversion of pressure units 149 torr to atm a. 1.47 b. 10.1 c. 0.196 d. 5.10
c. 0.196
determine the pressure exerted by 2.26mol of a gas in a 2.92L container at 32C a. 2.03 atm b. 56.6 atm c. 19.4 atm d. 5.93 atm
c. 19.4 atm
the specific heat capacity of aluminum is 0.89J/gC. Calculate the amount of energy needed to warm 4.33x10^3g of aluminum from 73C to 155C a. 8.8x10^2 kJ b. 6x10^2 kJ c. 3.2x10^2 kJ
c. 3.2x10^2 kJ
561.2J of heat was added to 8g of water. The final temperature of the water was measured to be 64.2C. what was the initial temperature of the water? a. -81C b. 81C c. 47.4C d. 3.61C
c. 47.4C
express 3.27x10^5 J in kilocalories a. 1.37x0^6 kcal b. 7.82x10^4 kcal c. 78.2 kal d. 327 kcal
c. 78.2 kal
the maximum number of electrons in the second principal energy level of an atom is a. 2 b. 6 c. 8 d. 18
c. 8
The least electronegative element of those listed is a. O b. Pb c. Ba d. Cu
c. Ba
SI units for specific heat capacity a. cal b. cal/g c. J/gC d. g/mL
c. J/gC
Choose the correct Lewis structure for the OH- ion a. [:O: H] - b. [O : H] - c. [ ::O:: H]-
c. [ ::O:: H]-
The elements chlorine and iodine have similar chemical properties because they a. are both metals b. are in the same chemical period c. have the same number of electrons in their outer energy levels
c. have the same number of electrons in their outer energy levels
heat is typically measured in a. Celsius b. F c. joules d. grams
c. joules
if atom X forms a diatomic molecule with itself, the bond is a. ionic b. polar covalent c. nonpolar covalent d. polar coordinate covalent
c. nonpolar covalent
Which color of visible light has the highest frequency a. red b. blue c. violet
c. violet
the alkaline earth metals have how many valence electrons a. 8 b. 7 c. 3 d. 2
d. 2
which of the following is the highest energy orbital for a silicon atom a. 1s b. 2s c. 3s d. 3p
d. 3p
what is the volume of a helium ballon that contains 1.95 mol helium at 27C and 1.10 atm a. 3.93L b. 39.7 L c. 48L d. 43.6L
d. 43.6L
the maximum number of electrons allowed in the p sublevel of the third principal level is a. 1 b. 2 c. 3 d. 6
d. 6
A given set of f orbitals consists of ___ orbitals a. 1 b. 3 c. 5 d. 7
d. 7
The noble gases contain how many valence electrons? a. 1 b. 7 c. 0 d. 8
d. 8
calculate the heat given off when 159.7g of copper cools from 155C to 23C. The specific heat capacity of copper is 0.385J/gC a. 1.14x10^3 b. 9.53x10^3 c. 5.48x10^4 d. 8.12x10^3
d. 8.12x10^3
which of the following bonds would be the most polar without being considered ionic a. Mg-O b. C-O c. O-O d. Si-O
d. Si-O
what is the expected ground-state electron configuration for Te2- a. [Kr]5s^2 5d^10 5p^4 b. [Kr]5s^2 4d^10 5p^4 c. [Kr]5s^2 4d^10 4f^14 5p^6 d. [Kr]5s^2 4d^10 5p^6
d. [Kr]5s^2 4d^10 5p^6
which of the following processes is exothermic (out of system) a. rolling a ball up a hill b. boiling water in a beaker to make steam c. allowing meat to thaw after taking it out of the freezer d. reacting hydrogen and oxygen gases to make water
d. reacting hydrogen and oxygen gases to make water
convert 3.00x10^2 atm to torr a. 3.04x10^4 torr b. 0.395 torr c. 20.8 torr d. 4.42x10^4 torr e. 2.28x10^5 torr
e. 2.28x10^5 torr
5.55kcal of energy is equivalent to how many J? a. 23.2J b. 2.32x10^-2 J c. 1.33J d. 0.754J e. 2.32x10^4J
e. 2.32x10^4J
the specific heat capacity of iron is 0.45 J/gC. How many joules of energy are needed to warm 1.31g of iron from 20C to 29C a. 17J b. 12J c. 26J d. 11J e. 5.3J
e. 5.3J
2116.16J of energy is equivalent to how many calories a. 1.97717x10^-3 cal b. 0.5057774 cal c. 2.11616 cal d. 2120.34 cal e. 505.774 cal
e. 505.774 cal
How much energy will be needed to heat 69.7 gal of water from 22C to 110C? (note that 1.00gal weighs 3.77 kg and that water has a specific heat capacity of 4.184J/gC. a. 9.67x10^7 kJ b. 2.57x10^4 kJ c. 2.57x10^7 kJ d. 2.31x10^4 kJ e. 9.67x10^4 kJ
e. 9.67x10^4 kJ
which of the following has the smallest atomic radius a. As b. Sb c. Bi d. P e. N
e. N
Rank the following bonds from least polar to most polar . Si-Cl P-Cl Mg-Cl S-Cl a. S-Cl P-Cl Mg-Cl Si-Cl b. P-Cl S-Cl Si-Cl Mg-Cl c. Mg-Cl Si-Cl P-Cl S-Cl d. Mg-Cl S-Cl P-Cl Si-Cl e. S-Cl P-Cl Si-Cl Mg-Cl
e. S-Cl P-Cl Si-Cl Mg-Cl
the color of a polar bear's fur is a. white b. brown c. black d. yellow e. colorless
e. colorless
___ is the ability to do work or produce heat a. gravity b.temperature c.radiation d.matter e. energy
e. energy