AP CHEM - tests/quizzes
What is the concentration (M) of 39.88 mL of an unknown NaOH solution if it required of to neutralize?
0.7617
There are ________ unpaired electrons in a ground state fluorine atom.
1
The energy of a photon that has a frequency of 1.821 × 1016 s-1 is ________ J.
1.21 × 10-17
How many moles of carbon monoxide are there in 36.55 g of carbon monoxide?
1.305
A sample of aluminum metal absorbs 11.2 J of heat, upon which the temperature of the sample increases from 23.2 °C to 30.5 °C. Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is ________ g.
1.7
There are ________ hydrogen atoms in 25 molecules of C4H4S2.
100
1 kilogram = ________ milligrams
1000000
The temperature of a 35.1 g sample of iron increases from to If the specific heat of iron is how many joules of heat are absorbed?
115 J
The temperature of a 11.8 g sample of calcium carbonate [CaCO3 (s)] increases from to If the specific heat of calcium carbonate is how many joules of heat are absorbed?
130 J
The formula weight of ammonium sulfate ((NH4)2SO4), rounded to the nearest integer, is ________ amu.
132
Given the following reactionsN2 (g) + 2O2 (g) → 2NO2 (g) ΔH = 66.4 kJ 2NO (g) + O2 (g) → 2NO2 (g) ΔH = -114.2 kJ the enthalpy of the reaction of the nitrogen to produce nitric oxideN2 (g) + O2 (g) → 2NO (g)
180.6 kJ
The ground state electron configuration of Ga is ________.
1s22s22p63s23p64s23d104p1
When the following equation is balanced, the coefficients are ________. C8H18 + O2 → CO2 + H2O
2, 25, 16, 18
When the following equation is balanced, the coefficients are ________.Al(NO3)3 + Na2S → Al2S3 + NaNO3
2, 3, 1, 6
Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:CaO (s) + H2O (l) → Ca(OH)2 (s)A 3.50-g sample of CaO is reacted with 3.38 g of H2O. How many grams of water remain after completion of reaction?
2.25
The wavelength of light that has a frequency of 1.20 × 1013 s-1 is ________ m.
2.5 x 10^-5
Magnesium and nitrogen react in a combination reaction to produce magnesium nitride:3 Mg + N2 → Mg3N2In a particular experiment, a 8.33-g sample of N2 reacts completely. The mass of Mg consumed is ________ g.
21.7
How many milliliters of 0.188 M HClO4 solution are needed to neutralize 50.00 mL of 0.0832 M NaOH?
22.1
The formula weight of Zn(ClO4)2 is ________ amu.
264.1
The formula weight of PbCO3 is ________ amu.
267.2
Calculate the percentage by mass of oxygen in Pb(NO3)2.
29
The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of of lead from 22 °C to 37 °C?
29 J
The formula weight of potassium dichromate (K2Cr2O7) is ________ amu.
294.18
The temperature of 25 °C is ________ in Kelvins.
298
The number 0.0101 has ________ significant figures.
3
When the following equation is balanced, the coefficient of oxygen is ________. PbS (s) + O2 (g) → PbO (s) + SO2 (g)
3
Electromagnetic radiation travels through vacuum at a speed of ________ m/s.
3.00 x 10^8
The output of a plant is 4335 pounds of ball bearings per week (five days). If each ball bearing weighs 0.0113 g, how many ball bearings does the plant make in a single day? (Indicate the number in proper scientific notation with the appropriate number of significant figures.)1 lb = 453.6 grams
3.48 × 107
What is the mass % of carbon in dimethylsulfoxide (C2H6SO) rounded to three significant figures?
30.7
The mass % of F in the binary compound KrF2 is ________.
31.20
Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide:Pb2+ (aq) + 2I- (aq) → PbI2 (s)Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 0.600 mol of Pb(NO3)2 (aq) to completely precipitate the lead?
338
The value of ΔH° for the reaction below is -72 kJ. ________ kJ of heat are released when 80.9 grams of HBr is formed in this reaction.H2 (g) + Br2 (g) → 2HBr (g)
36
How many Significant Figures does the number 0.005000 have?
4
When the following equation is balanced, the coefficients are ________. NH3 (g) + O2 (g) → NO2 (g) + H2O (g)
4, 7, 4, 6
The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is ________ M sodium ion and ________ M sulfate ion.
4.208, 2.104
Calculate the number of grams of solute in 500.0 mL of 0.159 M KOH.
4.46
What mass (g) of AgBr is formed when of AgNO3 is treated with an excess of aqueous hydrobromic acid?
4.59
Ham radio operators often broadcast on the 6-meter band. The frequency of this electromagnetic radiation is ________ MHz.
50
The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 38.5 g of O2 (g) reacts with excess CO.2CO (g) + O2 (g) → 2CO2 (g)
580 kj
How many grams of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium chloride?
6.11
What is the mass in grams of 2.00 × 105 atoms of naturally occurring neon?
6.67 x 10^-18
How many grams of calcium cyanide (Ca(CN)2) are contained in 0.69 mol of calcium cyanide?
61
Calculate the percentage by mass of lead in Pb(NO3)2.
62.6
There are ________ molecules of methane in 0.123 mol of methane (CH4).
7.40 × 10^22
What is the frequency of light (s-1) that has a wavelength of 3.86 × 10-5 cm?
7.77 × 1014 s-1
What is the wavelength of light (nm) that has a frequency of 3.22 × 1014 s-1?
932 nm
aluminum nitrate
Al(NO3)3
Predict the product in the combination reaction below.Al (s) + N2 (g) → ________
AlN
A compound that is composed of only carbon and hydrogen contains 85.7% C and 14.3% H by mass. What is the empirical formula of the compound?
CH2
The balanced net ionic equation for precipitation of CaCO3 when aqueous solutions of Na2CO3 and CaCl2 are mixed is ________.
Ca+(aq) + CO32- (aq) → CaCO3 (s)
Copper (II) Chloride
CuCl2
A one degree of temperature difference is the smallest on the ________ temperature scale.
Fahrenheit
Which of the following are strong acids? HI HNO3HF HBr
HI, HNO3, HBr
What are the spectator ions in the reaction between KOH (aq) and HNO3 (aq)?
K+ and NO3-
_________ is the abbreviation for the prefix mega-.
M
What are the spectator ions in the reaction between Mg(OH)2 (aq) and HCl (aq)?
Mg 2+ and Cl-
magnesium phosphate
Mg3(PO4)2
nitrogen tetroxide
NO4
sodium sulfide
Na2S
Ti2(SO4)3
Titanium (III) Sulfate
Which one of the following compounds is insoluble in water?
ZnS
The ground-state configuration of fluorine is ________.
[He]22s22p5
A small amount of salt dissolved in water is an example of a _______
a homogenous mixture
Elements in the modern version of the periodic table are arranged in order of increasing ________.
atomic number
percent abundance(amu) + percent abundance(amu)
average atomic mass
Objects can possess energy as ________. (a) endothermic energy (b) potential energy (c) kinetic energy
b and c
Ba(OH)2
barium hydroxide
How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?
c. 1.31
equation for speed of light
c=λv
CaBr2
calcium bromide
Sodium is much more apt to exist as a cation than is chlorine. This is because ________.
chlorine has a greater ionization energy than sodium does
If matter is uniform throughout and cannot be separated into other substances by physical processes, but can be decomposed into other substances by chemical processes, it is called a(n) ________.
compound
Solids have a ________ shape and are not appreciably ________.
definite, compressible
The energy of a photon of light is ________ proportional to its frequency and ________ proportional to its wavelength.
directly, inversely
Of the following, ________ radiation has the shortest wavelength. a. ultraviolet b. microwave c. radio d. infrared e. X-ray
e. X ray
In the Bohr model of the atom, ________.
electron energies are quantized
is boiling soup and melting ice endothermic or exothermic?
endothermic
A chemical reaction that absorbs heat from the surroundings is said to be ________ and has a ________ ΔH at constant pressure.
endothermic, positive
is the condensation of water vapor endothermic or exothermic?
exothermic
The reaction4Al (s) + 3O2 (g) → 2 Al2O3 (s) ΔH° = -3351 kJ is ________, and therefore heat is ________ by the reaction.
exothermic, released
A combination of sand, salt, and water is an example of a ________.
heterogenous mixture
For which of the following can the composition vary?
homogenous and heterogenous mixtures
(i) 1s2 2s2 2p6 3s1 (ii) 1s2 2s2 2p6 3s2 (iii) 1s2 2s2 2p6 3s2 3p1 (iv) 1s2 2s2 2p6 3s2 3p4 (v) 1s2 2s2 2p6 3s2 3p5The electron configuration belonging to the atom with the highest second ionization energy is ________.
i
Consider the following electron configurations to answer the questions that follow: (i) 1s2 2s2 2p6 3s1 (ii) 1s2 2s2 2p6 3s2 (iii) 1s2 2s2 2p6 3s2 3p1 (iv) 1s2 2s2 2p6 3s2 3p4 (v) 1s2 2s2 2p6 3s2 3p5The electron configuration that belongs to the atom with the lowest second ionization energy is ________.
ii
Electronegativity ________ from left to right within a period and ________ from top to bottom within a group.
increases, decreases
A strong electrolyte is one that ________ completely in solution.
ionizes
Fe2O3
iron (III) oxide
The gold foil experiment performed in Rutherford's lab ________.
led to the discovery of the atomic nucleus
A spectrum containing only specific wavelengths is called a(n) ________ spectrum.
line
According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the position and the ________ of an electron.
momentum
Of the following transitions in the Bohr hydrogen atom, the ________ transition results in the emission of the lowest-energy photon.
n = 6 → n = 3
A ________ ΔH corresponds to an ________ process.
negative, exothermic
When a hydrocarbon burns in air, what component of air reacts?
oxygen
ΔH for an endothermic process is ________ while ΔH for an exothermic process is ________.
positive, negative
P4O10
tetraphosphorus decoxide
CO, CO2 is an example of _________
the law of multiple proportions
How many significant figures does 0.0050 have?
two
(i) 1s2 2s2 2p6 3s1 (ii) 1s2 2s2 2p6 3s2 (iii) 1s2 2s2 2p6 3s2 3p1 (iv) 1s2 2s2 2p6 3s2 3p4 (v) 1s2 2s2 2p6 3s2 3p5The electron configuration of the atom with the most negative electron affinity is ________.
v
In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l)△H = -890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.
-100.1 kJ
The value of ΔH° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is ________ kJ.2S (s) + 3O2 (g) → 2SO3 (g)
-12
What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient water to give 350 mL of solution?
.45
"Absolute zero" refers to ________.
0 Kelvin
A 1.36-g sample of magnesium nitrate, Mg(NO3)2, contains ________ mol of this compound.
0.00917
How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?
0.0800
The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is ________.
0.0879
Lithium and nitrogen react to produce lithium nitride:6Li (s) + N2 (g) → 2Li3N (s)How many moles of N2 are needed to react with 0.550 mol of lithium?
0.0917
Lithium and nitrogen react to produce lithium nitride:6Li (s) + N2 (g) → 2Li3N (s)How many moles of lithium nitride are produced when 0.330 mol of lithium react in this fashion?
0.110
A solution is prepared by mixing 15.0 mL of 0.100 M HCl and 5.00 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?
0.125
Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride:Ag+ (aq) + Cl- (aq) → AgCl (s)Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.149 M AgNO3 solution to completely precipitate the silver?
0.218
A 22.5-g sample of ammonium carbonate contains ________ mol of ammonium ions.
0.467
The concentration (M) of an aqueous methanol produced when 0.200 L of a 2.00 M solution was diluted to 0.800 L is ________.
0.500
