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a 2 KClO3(s) 2 KCl(s) + 3 O2(g) You get 1 point if you have the above equation b (2/3 mole KClO3) (3 moles O2/2 moles KClO3) = 1 mole O2 You get 1 point for the correct answer and 1 point for the work You can get these points if you correctly use information from an incorrect equation in part a c At STP the volume of 1 mole of O2 should be 224 liters The volume is greater because oxygen was not the only gas in the sample Water vapor was present The presence of the additional gas leads to a larger volume You get 1 point for discussing STP and 224 liters, and 1 point for discussing the presence of water vapor d There are two acceptable equations; either will get you 1 point You do not need both equations
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Gases 121
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S(s) + O2(g) SO2(g) 2 S(s) + 3 O2(g) 2 SO3(g) If you chose the first equation, the moles of gas produced would be: (1 mole O2) (1 mole SO2/1 mole O2) = 1 mole SO2 If you chose the second equation, the moles of gas produced would be: (1 mole O2) (2 mole SO3/3 mole O2) = 2/3 mole SO2 You get 1 point for either of these solutions You will also get 1 point if you used an incorrect number of moles of O2 from a wrong answer for part b e Either of the possible sulfur oxides will dissolve in water to produce an acid This will get you 1 point, as will a similar comment and either of the following equations: SO2 + H2O H2SO3 SO3 + H2O H2SO4 Total your points for the different parts There are 8 points possible
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U Rapid Review
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Kinetic Molecular Theory Gases are small particles of negligible volume moving in a random straight-line motion, colliding with the container walls (that is the gas pressure) and with each other During these collisions no energy is lost, but energy may be transferred from one particle to another; the Kelvin temperature is proportional to the average kinetic energy There is assumed to be no attraction between the particles Pressure Know how a barometer operates and the different units used in atmospheric pressure Boyle s law The volume and pressure of a gas are inversely proportional if the temperature and amount are constant Charles s law The volume and temperature of a gas are directly proportional if the amount and pressure are constant Gay-Lussac s law The pressure and temperature of a gas are directly proportional if the amount and volume are constant Combined gas law Know how to use the combined gas equation P1V1/T1 = P2V2/T2 Avogadro s law The number of moles and volume of a gas are directly proportional if the pressure and temperature are constant Remember that 1 mol of an ideal gas at STP(1 atm & 0 C) occupies a volume of 224 L Ideal gas equation Know how to use the ideal gas equation PV = nRT Dalton s law The sum of the partial pressures of the individual gases in a gas mixture is equal to the total pressure: PTotal = PA + PB + Pc + Graham s law The lower the molecular mass of a gas, the faster it will effuse/diffuse r M2 Know how to use Graham s law: 1 = r2 M1
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122 U Step 4 Review the Knowledge You Need to Score High
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Gas stoichiometry Know how to apply the gas laws to reaction stoichiometry problems Non-ideal gases Know how the van der Waals equation accounts for the non-ideal behavior of real gases Tips Make sure the temperature is in kelvin; gas laws are being applied to gases only; the units cancel; and the answer is reasonable
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