AP Chemistry Practice Questions
25.0 L of hydrogen gas at 50.0 atm and 25 degrees Celsius expands to 65.0 L and is subsequently heated to 35 degrees Celsius. What is the new pressure? a) 19.9 atm b) 25.2 atm c) 26.9 atm d) 28.4 atm e) 31.2 atm
a
A bicycle tire is filled to a pressure of 4.42 atm (65 psi) at a temperature of 12 degrees Celsius. If the temperature increases to 33 degrees Celsius, what is the pressure in the tire? Assume the volume of the tire is constant. a) 4.75 atm b) 5.91 atm c) 9.28 atm d) 12.1 atm e) 16.1 atm
a
A volatile compound with a mass of 0.8822 grams is placed in an evacuated 0.250 L flask. The flask is heated to evaporate the compound. At 99 degrees Celsius, the pressure in the flask is 1.25 atm. What is the molar mass of the compound? a) 86.2 g/mol b) 116 g/mol c) 229 g/mol d) 257 g/mol e) 303 g/mol
a
According to the Arrhenius acid-base definition a) acids produce H^+ in aqueous solutions and bases produce OH^- in aqueous solutions b) acids produce OH^- in aqueous solutions and bases produce H^+ in aqueous solutions c) acids only react with bases d) all hydrogen halides are strong acids e) acids and bases are strong electrolytes
a
All of the following are exact conversions EXCEPT a) 1 pound=453.6 g b) 1 m^3=1x10^3 L c) 1 cm^3=1 mL d) 2.54 cm=1 inch e) 1 kg=1x10^3 g
a
An element has three naturally occurring isotopes with the following abundances and masses: abundance: 78.99%, mass (amu): 23.985042 abundance: 10.00%, mass (amu): 24.985837 abundance: 11.01%, mass (amu): 25.982593 Determine the atomic mass of the element a) 24.31 b) 24.98 c) 74.95 d) 2431 e) none of the above
a
At 108 degrees Celsius, the pressure in a 10.0 L flask is 874 mm Hg. How many moles of gas are in the flask? a) 0.368 mol b) 0.873 mol c) 1.30 mol d) 348 mol e) 986 mol
a
How many moles of ammonia can be made by reacting 7.0 moles of N2 with 4.0 moles of H2? N2(g) + 3H2(g) -> 2NH3(g) a) 2.7 mol b) 4.0 mol c) 7.0 mol d) 11 mol e) 14 mol
a
Isopentyl acetate, a molecule composed of C, H, and O, smells like bananas. Combustion analysis of 1.750 grams of this molecule yields 1.695 g H2O and 4.142 g CO2. What is the simplest formula for isopentyl acetate? a) C7H14O2 b) C7H7O4 c) C8H10O3 d) C8H16O e) C9H6O
a
The average molar mass of lithium is 6.941. A sample of lithium consists of two isotopes with masses of 6.01512 amu and 7.01600 amu. Determine the percent abundance of each isotope. a) 74.9% Li-6 and 92.51% Li-7 b) 8.45% Li-6 and 91.55% Li-7 c) 12.49% Li-6 and 87.51% Li-7 d) 91.55% Li-6 and 8.45% Li-7 e) 92.51% Li-6 and 7.49% Li-7
a
The gravity on the surface of Earth is 6.02 times greater than that on the moon. If an object has both a mass and weight of 1.00 kg on earth, on the moon the same object will have a) a mass of 1.00 kg and a weight of 0.166 kg b) a mass of 1.00 kg and a weight of 1.00 kg c) a mass of 1.00 kg and a weight of 6.02 kg d) a mass of 0.166 kg and a weight of 0.166 kg e) a mass of 0.166 kg and a weight of 1.00 kg
a
The molar mass of helium and oxygen are 4.0g/mol and 16g/mol, respectively. At the same temperature and pressure, 1 mole of helium will occupy a) the same volume as 1 mole of oxygen b) four times the volume of 1 mole of oxygen c) twice the volume of 1 mole of oxygen d) half the volume of 1 mole of oxygen e) one fourth the volume of 1 mole of oxygen
a
Vinegar is a homogeneous mixture of two liquids: acetic acid and water. Which method is best for separating the components of vinegar? a) distillation b) filtration c) electrolysis d) gas-liquid chromatography e) light absorption
a
What is the correct formula for potassium dichromate? a) K2Cr2O7 b) K2(Cr2O7)2 c) K2CrO4 d) (K2CrO4)2 e) KCrO4
a
What is the correct name for Ag2O? a) silver (I) oxide b) silver (I) monoxide c) silver (II) oxide d) silver dioxide e) disilver monoxide
a
What is the correct name for HI (aq)? a) hydroiodic acid b) hydrogen iodide ion c) monohydrogen monoiodide d) iodate acid e) iodine hydride
a
What is the correct name for PF5? a) phosphorous pentafluoride b) phosphorous (V) fluoride c) phosphorofluoride d) pentafluorophosphorus e) pentafluorophosphate
a
When HCl(g) and NH3(g) are mixed, a white solid forms. What is the balanced equation for this reaction? a) HCl(g) + NH3(g) -> NH4Cl(s) b) HCl(g) + NH3(g) -> NH2Cl(g) + H2(s) c) HCl(g) + NH3(g) -> NH4(s) + Cl(g) d) HCl(g) + NH3(g) -> NH2Cl(s) + H2(g) e) 3HCl(g) + NH3(g) -> NCl3(s) + 3H2(g)
a
Which method is correct for determining the mass of carbon dioxide that can be made by the combustion of 3.219 grams of ethanol with excess oxygen? C2H5OH(l) + 3O2(g) -> 2CO2(g) + 3H2O(l) a) 3.219 g C2H5OH (1 mole/46.07g)(2 mole CO2/1 mole C2H5OH)(44.01g CO2/1 mole) b) 3.219 g C2H5OH (1 mole/46.07g)(1 mole CO2/2 mole C2H5OH)(44.01g CO2/1 mole) c) 3.219 g C2H5OH (1 mole/46.07g)(1 mole CO2/1 mole C2H5OH)(44.01g CO2/1 mole) d) 3.219 g C2H5OH (46.07 mole/1g)(2 mole CO2/1 mole C2H5OH)(44.01g CO2/1 mole) e) 3.219 g C2H5OH (46.07 mole/1g)(1 mole CO2/2 mole C2H5OH)(44.01g CO2/1 mole)
a
Which of the following samples contains the largest number of hydrogen atoms? a) 2.0 moles of C6H16 b) 3.0 moles of C3H8 c) 4.0 moles of C3H6 d) 6.0 moles of C2H4 e) 8.0 moles of C2H2
a
Which two of the ions below have the same number of electrons? (top:127, bottom:53) I^1-, (top:119, bottom:50) Sn^2+, (top:207, bottom:82) Pb^2+ (top:207, bottom:82) Pb^4+ (top:137, bottom:56) Ba^2+ a) (top:127, bottom:53) I^1- and (top:137, bottom:56) Ba^2+ b) (top:127, bottom:53) I^1- and c) top:207, bottom:82) Pb^2+ and (top:137, bottom:56) Ba^2+ d) (top:119, bottom:50) Sn^2+ and (top:137, bottom:56) Ba^2+ e) top:207, bottom:82) Pb^2+ and (top:207, bottom:82) Pb^4+
a
Write a balanced net ionic equation for the reaction of aluminum hydroxide, Al(OH)3, with nitric acid. a) Al(OH)3(s) + 3H^+(aq) -> Al^3+(aq) + 3H2O b) Al(OH)3(s) + 3H^+(aq) -> AlH3(s) + 3OH^-(aq) c) (OH)3(aq) + 3H^+(aq) -> 3H2O d) 3OH^-(aq) + 3H^+(aq) -> 3H2O e) Al^3+(aq) + 3NO3^-(aq) -> Al(NO3)3(aq)
a
A 1.45 g sample of chromium contains _____ atoms. a) 1.25x10^22 b) 1.6x10^22 c) 8.73x10^23 d) 2.16x10^25 e) 4.54x10^25
b
A 3.00 L flask contains 2.33 g of argon gas at 312 mm Hg. What is the temperature of the gas? a) 151 K b) 257 K c) 292 K d) 341 K e) 4890 K
b
A mass of 5.0 grams of dry ice, CO2(s), is sealed in an evacuated 2.0 L plastic soda bottle. What is the pressure inside the bottle when the CO2 is heated to 35 degrees Celsius? a) 0.16 atm b) 1.4 atm c) 8.9 atm d) 18 atm e) 63 atm
b
A strontium ion has ____ electrons. a) 35 b) 36 c) 37 d) 38 e) 39
b
All of the following groups are considered main group elements EXCEPT a) group 2 b) group 7 c) group 14 d) group 17 e) group 18
b
An aqueous solution of copper sulfate is blue. This solution absorbs a) blue light b) red light c) only infrared light d) only ultraviolet light e) only light with wavelengths shorter than 400 nm
b
Assign oxidation numbers to each atom in manganese(IV) oxide. a) Mn=+4;O=0 b) Mn=+4;O=-2 c) Mn=+2;O=0 d) Mn=+2;O=-2 e) Mn=0;O=0
b
How many nonmetals, metalloids, and metals are in group 14? a) 0 nonmetals, 3 metalloids, and 2 metals b) 1 nonmetals, 2 metalloids, and 2 metals c) 2 nonmetals, 2 metalloids, and 1 metals d) 2 nonmetals, 1 metalloids, and 2 metals e) 3 nonmetals, 0 metalloids, and 2 metals
b
How many significant figures are in the following mass: 0.00047800 kg? a) 3 b) 5 c) 6 d) 8 e) 9
b
Identify the ions and their charges in Mg3N2 a) Mg^+, N^3- b) Mg^2+, N^3- c) Mg^3+, N^2- d) Mg3^2+, N2^3- e) Mg3^6+, N2^6-
b
Identify the ions and their charges in Na2SO4. a) Na^+, SO4^- b) Na^+, SO4^2- c) Na^+, SO^4- d) Na^2+, SO^4- e) Na^2+, SO4^2-
b
If 16.4 g of oxygen gas react with excess hydrogen, what mass of water is produced? 2H2(g) + O2(g) -> 2H2O(g) a) 9.23 g b) 18.5 g c) 20.4 g d) 23.9 g e) 36.9 g
b
If 17 g MgCl2 is dissolved in 5.0 L of water, what is the chloride ion molarity in the solution? a) 0.036 M b) 0.071 M c) 0.68 M d) 0.77 M e) 7.8 M
b
If the volume of a confined gas is doubled at constant temperature, what change is observed? a) the pressure of the gas is decreased to 1/4 of its original value b) the pressure of the gas is decreased to 1/2 of its original value c) the pressure of the gas is increased to twice its original value d) the density of the gas is doubled e) the velocities of the molecules are doubled
b
Many experiments are conducted at 298 K. What is this temperature in Celsius? a) 0 C b) 25 C c) 55 C d) 273 C e) 298 C
b
The mass of a single atom of sulfur is 5.325x10^-23 grams. Which is a correct method for determining molar mass of elemental sulfur, S8? a) (5.325x10^-23 g S/1 atom)(1 atom/6.022x10^23 moles)(1 mole S8/ 8 mole S) b) (5.325x10^-23 g S/1 atom)(6.022x10^23 atoms/1 mole S)(8 mole S/1 mole S8) c) (5.325x10^-23 g S/1 atom)(1 atom/6.022x10^23 moles)(8 mole S/1 mole S8) d) (1 atom/5.325x10^-23 g S)(6.022x10^23 moles/1 atom)(1 mole S8/ 8 mole S) e) (5.325x10^-23 g S/1 atom)(6.022x10^23 atoms/1mole S)(1 mole S8/ 8 mole S)
b
What is the correct answer to the expression below? 2.54cm/inch x (182.3 inch - 179.219 inch) a) 8 cm b) 7.8 cm c) 7.83 cm d) 7.826 cm e) 7.8257 cm
b
What is the correct formula for chromium (II) nitrate? a) Cr3NO3 b) Cr(NO3)3 c) Cr2(NO3)3 d) Cr3(NO3)2 e) Cr3(NO3)3
b
What is the correct formula for sulfur dichloride? a) SCl b) SCl2 c) S2Cl d) S2Cl2 e) S4Cl2
b
What is the density of argon gas at 25 degrees Celsius and 1.00 atm? a) 0.0110 g/L b) 1.63 g/L c) 19.5 g/L d) 977 g/L e) 1.24 x 10^3 g/L
b
What is the reduction half-reaction for the equation below? 5Fe^2+(aq) + MnO4^-(aq) + 8H^+(aq) -> 5Fe^3+(aq) + Mn^2+(aq) + 4H2O a) MnO4^-(aq) + 5e^- -> Mn^2+(aq) + 2O2(g) b) MnO4^-(aq) + 8 H^+(aq) +5e^- -> Mn^2+(aq) + 4H2O c) Fe^2+(aq) + e^- -> Fe^3+(aq) d) 8H^+(aq) + 8e^- -> 8H2O e) none of the above
b
Which of the following ionic compounds are likely to be soluble in water: Mg(OH)2, Pb(NO3)2, AgI, Na2CO3, and Cu3(PO4)3? a) Na2CO3 only b) Pb(NO3)2 and Na2CO3 c) Mg(OH)2, Na2CO3, and Cu3(PO4)3 d) Mg(OH)2, AgI ,and Cu3(PO4)3 e) Pb(NO3)2, AgI, Na2CO3, and Cu3(PO4)3
b
Which species has 63 neutrons? a) (top:112, bottom:48) Cd b) (top:112, bottom:49) In c) (top:63, bottom:29) Zn d) (top:152, bottom:63) Eu e) none of the above
b
You have a 5.0 g sample of each of the following elements: Ra, Rb, Rh, Rn, Ru. Which sample contains the most atoms? a) Ra b) Rb c) Rh d) Rn e) Ru
b
A mass of 12.0 g of calcium chloride is diluted to a volume of 250 mL in a volumetric flask. Which of the equations below is a correct method for determining the chloride ion concentration? a) (12.0g CaCl2/250 mL)(1000mL/1 L)(1 mole CaCl2/111.0 g) b) (12.0g CaCl2/250 mL)(1L/1000mL)(1 mole CaCl2/111.0 g)(2 mole Cl-/1 mole CaCl2) c) (12.0g CaCl2/250 mL)(1000mL/1L)(1 mole CaCl2/111.0 g)(2 mole Cl-/1 mole CaCl2) d) (12.0g CaCl2/250 mL)(1L/1000mL)(1 mole CaCl2/111.0 g)(1 mole CaCl2/2 mole Cl-) e) (12.0g CaCl2/250 mL)(1000mL/1L)(1 mole CaCl2/111.0 g)(1 mole CaCl2/2 mole Cl-)
c
All of the following are examples of chemical change EXCEPT a) the fermentation of wine b) the tarnishing of silver c) the condensation of steam d) the combustion of butane gas e) the rusting of iron
c
All of the following statements are false EXCEPT a) copper (Cu) is a homogeneous mixture of carbon (C) and uranium (U) b) table salt is a heterogeneous mixture of sodium metal and chlorine gas c) soda water is a homogeneous mixture of carbon dioxide gas and water d) sugar dissolves completely in water to give a heterogeneous mixture e) water (H20) is a homogeneous mixture containing hydrogen and oxygen
c
Gallium has an atomic mass of 69.7 amu. In a typical sample, 60.4% of Ga exists as Ga-69 (68.9257 amu). What is the identity and the atomic mass of the other isotope? a) (top:70, bottom:30) Ga; 70.9 amu b) (top:70, bottom:31) Ga; 70.9 amu c) (top:71, bottom:31) Ga; 70.9 amu d) (top:71, bottom:31) Ga; 71.9 amu e) (top:72, bottom:31) Ga; 71.9 amu
c
How many protons and electrons are in a sulfate ion, SO4^2-? a) 46 protons and 48 electrons b) 48 protons and 48 electrons c) 48 protons and 50 electrons d) 50 protons and 48 electrons e) none of the above
c
Identify all of the spectator ions in the precipitation reaction below. Ca^2+(aq) + 2Br^-(aq) + 2Li^+(aq) + CO3^2-(aq) -> CaCO3(s) + 2Li^+(aq) + 2Br^-(aq) a) Ca^2+ and Li^+ b) Br^- and CO3^2- c) Br^- and Li^+ d) CaCO3 e) Ca^2+, Br^-, Li^+, and CO3^2-
c
Identify the reaction type for the reaction between potassium metal and hydrochloric acid. 2K(s) + 2H^+(aq) -> 2K^+(aq) + H2(g) a) precipitation b) acid-base c) oxidation-reduction d) both a and c e) none of the above
c
In the laboratory, acid spills are often neutralized by adding sodium bicarbonate. What mass of sodium bicarbonate reacts with 225 mL of 6.00 M HCl? H^+(aq) + NaHCO3(s) -> H2O + CO2(g) + Na^+(aq) a) 1.35 g b) 71.5 g c) 113 g d) 143 g e) 2240 g
c
NH3(aq) is a a) strong base b) strong acid c) weak base d) weak acid e) neither an acid nor a base
c
Place the following units of pressure in order from lowest to highest pressure a) 1 atm<1 Pa<1 mm Hg<1 bar b) 1 mm Hg<1 bar<1 atm<1 Pa c) 1 Pa<1 mm Hg<1 bar<1 atm d) 1 Pa<1 mm Hg<1 atm<1 bar e) 1 bar<1 mm Hg<1 Pa<1 atm
c
What is the formula for chlorous acid? a) HCl b) HClO c) HClO2 d) HClO3 e) HClO4
c
What is the mass in grams of 0.362 moles nitric acid (HNO3)? a) 0.00574 g b) 0.0438 g c) 22.8 g d) 53.8 g e) 174 g
c
What mass of potassium ions is present in 25.0 mL of 0.50 M K2SO4? a) 0.250 g b) 0489 g c) 0.978 g d) 2.18 g e) 4.36 g
c
What volume of oxygen (O2) at 22 degrees Celsius and 1.00 atm contains the same number of molecules as 0.400 L H2 at 45 degrees Celsius and 1.00 atm? a) 0.251 L b) 0.298 L c) 0.371 L d) 0.400 L e) 0.431 L
c
Which of the following methods correctly describes the preparation of 1.00L of an aqueous solution of 0.500 M NaOH? a) place 0.500 g NaOH(s) in a flask and dilute to 1.00 L with water b) place 0.500 g NaOH(s) in a flask and add 1.00 L of water c) place 20.0 g NaOH(s) in a flask and dilute to 1.00 L with water d) place 20.0 g NaOH(s) in a flask and add 1.00 L of water e) place 40.0 g NaOH(s) in a flask and add 500 g of water
c
Which of the following samples contains the largest number of atoms? a) 2.0 moles of H3PO4 b) 3.0 moles of H2SO3 c) 4.0 moles of HNO3 d) 6.0 moles of HClO e) 8.0 moles of HBr
c
Which term best describes table salt (NaCl) at room temperature? a) gas b) element c) compound d) homogeneous mixture e) heterogeneous mixture
c
Write a balanced net ionic equation for the reaction of aqueous solutions of lead (II) nitrate and potassium chloride. a) Pb(NO3)2(aq) + 2KCl(aq) -> PbCl2(s) + 2 KNO3(aq) b) Pb^2+(aq) + 2K^+(aq) -> PbK2(s) c) Pb^2+(aq) + 2Cl^-(aq) -> PbCl2(s) d) NO3^-(aq) + K^+(aq) -> KNO3(s) e) no precipitation occurs
c
2.500 grams of MgSO4xH2O, a hydrated salt with an unknown water content, is dried in an oven to remove the water. After drying, the anhydrous salt has a mass of 1.221 grams. How many moles of water are present per mole of hydrated magnesium sulfate? a) 1 b) 3 c) 5 d) 7 e) 9
d
A 25.00 mL sample of vinegar is diluted with water to a final volume of 250.0 mL. A 25.00 mL portion of the diluted vinegar is then titrated with 0.0998 M NaOH. If 22.43 mL of NaOH is required to reach the equivalence point, what is the original concentration of acetic acid in the vinegar? CH3CO2H(aq) + OH^-(aq) -> CH3CO2^-(aq) + H2O a) 0.0538 M b) 0.0895 M c) 0.538 M d) 0.895 M e) 5.38 M
d
A reducing agent is a species that a) takes a proton from an Arrhenius acid b) is reduced in a chemical reaction c) gains electrons in a chemical reaction d) loses electrons in a chemical reaction e) gives a proton to an Arrhenius base
d
Express 4.220 x 10^2 mL in standard notation. a) 0.0422 mL b) 0.04220 mL c) 422 mL d) 422.0 mL e) 4220 mL
d
How many elements are contained in period 4? a) 3 b) 8 c) 10 d) 18 e) 32
d
If the outdoor temperature is 17.0 degrees Celsius, what is the temperature in Fahrenheit? a) -1.40 degrees Fahrenheit b) 30.6 degrees Fahrenheit c) 41.4 degrees Fahrenheit d) 62.6 degrees Fahrenheit e) 74.6 degrees Fahrenheit
d
The catalytic conversion of ammonia to nitric oxide is the first step in a three-step process which ultimately results in nitric acid. Balance the equation for the reaction. aNH3(g) + bO2(g) -> cNO(g) + dH2O(g) a) a=2, b=1, c=2, d=1 b) a=3, b=2, c=3, d=3 c) a=4, b=3, c=2, d=6 d) a=4, b=5, c=4, d=6 e) a=6, b=15, c=6, d=9
d
The mass of a single atom of ziroconium is 1.515x10^-22 grams. Which is a correct method for determining the molar mass of Zr. a) (1 g/1.515x10^-22 atoms)(1 atom/6.022x10^23 moles) b) (1 g/1.515x10^-22 atoms)(6.022x10^23 atoms/1 mole) c) (1.515x10^-22 g/1 atom)(1 atom/6.022x10^23 moles) d) (1.515x10^-22 g/1 atom)(6.022x10^23 atoms/1 mole) e) none of the above
d
What is a correct method for converting Celsius to kelvin? a) t(K)=9K/5C (tC-273.15C) b) t(K)=5K/9C (tC+273.15C) c) t(K)=1K/1C (tC-273.15C) d) t(K)=1K/1C (tC+273.15C) e) none of the above
d
What is the balanced net ionic equation for the neutralization of aqueous solutions of sodium hydroxide and perchloric acid, HClO4? a) OH^-(aq) + HClO4(aq) -> H2O + ClO4^-(aq) b) NaOH(aq) + H^+(aq) -> H2O + Na^+(aq) c) Na^+(aq) + ClO4^-(aq) -> NaClO4(s) d) OH^-(aq) + H^+(aq) ->H2O e) None of the above are correct
d
What is the balanced net ionic equation for the reaction between aqueous solutions of acetic acid and sodium hydroxide? a) CH3CO2H(aq) + OH^-(aq) -> CH3(aq) + CO3^2-(aq) + H2(aq) b) CH3CO2H(aq) + 3NaOH(aq) -> CCO2H^3-(aq) + 3Na^+(aq) + H2O c) CH3CO2H(aq) + OH^-(aq) -> CH3^-(aq) + CO2(g) + H2O d) CH3CO2H(aq) + OH^-(aq) -> CH3CO2^-(aq) + H2O e) CH3CO2H(aq) + 2Na^+(aq) + 2OH^-(aq) -> CH3CO2^2-(aq) + 2Na^+(aq) + H2O
d
What is the percent composition of iron (II) sulfate hexahydrate? a) 4.2% Fe; 4.2% S; 41.6% O; 50.0% H b) 16.7% Fe; 16.7% S; 66.6% O c) 21.5% Fe; 12.3% S; 24.6% O; 41.6% H d) 21.5% Fe; 12.3% S; 61.5% O; 4.7% H e) 36.8% Fe; 21.1% S; 42.1% O
d
What is the percent composition of silicon nitride (Si3N4)? a) 30.21% Si and 69.79% N b) 42.92% Si and 57.08% N c) 54.03% Si and 45.97% N d) 60.06% Si and 39.94% N e) 69.40% Si and 30.60% N
d
What mass of oxygen will react with 2.64 g of magnesium? 2Mg(s) + O2(g) -> MgO(s) a) 0.487 g b) 1.00 g c) 1.26 g d) 1.74 g e) 3.47 g
d
Which description most accurately describes neptunium-239? a) mass number=93, atomic number=239 b) mass number=93, number of neutrons=146 c) mass number=146, atomic number=93 d) number of protons=93, number of neutrons=146 e) number of protons=93, atomic number=239
d
Which list contains only strong acids? a) HCl, HNO3, HF, HClO4 b) H2SO4, H3PO4, HClO4, NH3 c) HCl, HNO3, H3PO4, HClO4 d) HCl, H2SO4, HClO4, HI e) HNO3, H2SO4, NaOH, H3PO4
d
Which one of the following statements concerning matter is correct? a) a gas has a fixed volume but not a rigid shape b) a liquid has a fixed volume and a rigid shape c) a liquid takes on both the volume and the shape of its container d) a solid has a fixed volume and a rigid shape e) both b and d are correct
d
Which two atoms below have the same number of neutrons? (top:15, bottom:8) O, (top:16, bottom:8) O, (top:20, bottom:9) F, (top:20, bottom:10) Ne, (top:22, bottom:11) Na a) (top:15, bottom:8) O and (top:16, bottom:8) O b) (top:16, bottom:8) O and (top:22, bottom:11) Na c) (top:20, bottom:9) F and (top:22, bottom:11) Na d) (top:20, bottom:9) F and (top:22, bottom:11) Na e) (top:20, bottom:10) Ne and (top:22, bottom:11) Na
d
A mass of 8.15 g C2H4(g) reacts with excess oxygen. If 16.2 g CO2(g) is collected, what is the percent yield of the reaction? C2H4(g) + 3O2(g) -> 2CO2(g) + 2H2O(g) a) 25.6% b) 31.7% c) 41.0% d) 57.1% e) 63.3%
e
All of the following statements are true EXCEPT a) of the 113 known elements, 91 occur naturally b) an element cannot be broken down into two or more pure substances c) a compound is a substance that contains two or more elements d) a pure compound always contains the same elements in the same mass percentages e) another name for a heterogeneous mixture is a solution
e
All of the following statements are true EXCEPT a) potassium is represented by the symbol K b) zinc is represented by the symbol Zn c) argon is represented by the symbol Ar d) iron is represented by the symbol Fe e) nitrogen is represented by the symbol Ni
e
Aluminum reacts with oxygen to form aluminum oxide. Which of the reactions below is correct and properly balanced? a) Al(s) + O(g) -> AlO(s) b) 2Al(s) + O(g) -> 2AlO(s) c) 3Al(s) + O(g) -> Al3O2(s) d) 4Al(s) + O(g) -> 2Al2O(s) e) 4Al(s) + 3O(g) -> 2Al2O3(s)
e
An intensive property is a) too small to be observed b) dependent only on mass and temperature c) visible to the human eye d) dependent upon amount e) independent of amount
e
Assign oxidation numbers to each atom in calcium perchlorate, Ca(ClO4)2. a) Ca=0; Cl=0; O=0 b) Ca=0; Cl=-1; O=-2 c) Ca=+2; Cl=-1; O=-2 d) Ca=+2; Cl=+5; O=-2 e) Ca=+2; Cl=+7; O=-2
e
Avogadro's law states that a) 1 liter of any gas contains 6.02 x 10^23 gas molecules b) the volume of a gas is directly proportional to its temperature c) the gas constant equals 0.0821 L x atm/(mol x K) for all gases d) the volume of a gas must always be constant e) equal volumes of all gases at the same pressure and temperature contain an equal number of moles
e
Beta particles have identical properties to a) helium atoms that have been stripped of their electrons b) elemental helium c) high energy radiation d) neutrons e) electrons
e
The combustion of methanol, CH3OH, yields carbon dioxide and water as products. Which of the reactions below is correct and properly balanced? a) CH3OH(l) + O2(g) -> CO2(g) + H2O(g) b) CH3OH(l) + O2(g) -> CO2(g) + 2H2O(g) c) 2CH3OH(l) + O2(g) -> 2CO2(g) + 4H2O(g) d) 2CH3OH(l) + 2O2(g) -> 2CO2(g) + 2H2O(g) e) 2CH3OH(l) + 3O2(g) -> 2CO2(g) + 4H2O(g)
e
The principle ingredient in Tums antacid tablets is calcium carbonate, CaCO3. A single tablet contains 0.500 g CaCO3. What volume of 0.2500 M HCl is required to titrate a tablet of Tums? 2H^+(aq) + CO3^2-(aq) -> H2O + CO2(g) a) 0.0100 mL b) 0.0200 mL c) 10.0 mL d) 20.0 mL e) 40.0 mL
e
What are the values for x and y, respectively, in CaxHyPO4? a) 1 and 2 b) 2 and 1 c) 1 and 3 d) 2 and 2 e) 1 and 1
e
What is the correct name for N203? a) nitrogen oxide b) nitrogen (II) oxide c) nitrogen (III) oxide d) trioxygen dinitride e) dinitrogen trioxide
e
What is the identity of (top:55, bottom:25) X? a) zinc b) silver c) iridium d) cesium e) manganese
e
What reaction occurs when aqueous solutions of magnesium nitrate and potassium iodide are mixed? a) Mg^2+(aq) + 2K^+(aq) -> MgK2(s) b) Mg^2+(aq) + 2I^-(aq) -> MgI2(s) c) NO3^-(aq) + K^+(aq) -> KNO3(s) d) Mg^2+(aq) + 2 NO3^-(aq) + 2K^+(aq) + 2I^-(aq) -> MgI2(s) + 2KNO3(s) e) no reaction occurs
e
Which group of three elements contains a transition metal, a halogen, and a noble gas? a) S, I, Cu b) Br, Kr, Ba c) Ar, Hg, Rn d) Ce, N, He e) Cu, I, Xe
e
Which is a correct expression for converting Celsius to Fahrenheit? a) degrees Fahrenheit=(5F/9C) tC-32F b) degrees Fahrenheit=(5F/9C) tC+32F c) degrees Fahrenheit=(5F/9C) (tC+32F) d) degrees Fahrenheit=(9F/5C) tC-32F e) degrees Fahrenheit=(9F/5C) tC+32F
e
Which method is best for removing the pulp from orange juice? a) distillation b) light absorption c) electrolysis d) gas-liquid chromatography e) filtration
e
Which of the following methods is correct for calculating the moles of Al^3+ in 125 mL of 0.234 M Al(NO3)3? a) (0.234 mol Al(NO3)3/125 mL)(1000 mL/1 L)(1 mol Al^3+/1 mol Al(NO3)3) b) (0.234 mol Al(NO3)3/125 mL)(1000 mL/1 L)(1 mol Al^3+/3 mol Al(NO3)3) c) 125 mL(1 L/1000 mL)(0.234 mol Al(NO3)3/1 L)(1 mol Al^3+/3 mol Al(NO3)3) d) 125 mL(1000 mL/1 L)(1 L/0.234 mol Al(NO3)3)(1 mol Al^3+/1 mol Al(NO3)3) e) 125 mL(1 L/1000 mL)(0.234 mol Al(NO3)3/1 L)(1 mol Al^3+/1 mol Al(NO3)3)
e
