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All reactions are shown in terms of the reduction reaction relative to the standard hydrogen electrode. The more positive the value of the voltage associated with the half-reaction (E ), the more readily the reaction occurs. The strength of the oxidizing agent increases as the value becomes more positive, and the strength of the reducing agent increases as the value becomes more negative.

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know. Past experience also affects your confidence (positive or negative) on different test types. Personally, I like questions that have one answer. Period. Too many choices make me less, rather than more, comfortable. I had an environmental science professor in college that wrote multiple-choice questions with the answers: (a) never true, (b) moderately true, (c) true, (d) often false, and (e) always false. Picking the right answer was excruciating and confused me so much I didn t feel fairly tested on my true knowledge level. However, some people are great at eliminating red herrings offered in multiple-choice questions and sail through without breaking a sweat. Here is how they do it. Multiple-choice questions have three parts:

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8 C Using Dalton s law (PTotal = PA + PB + ), the partial pressure may be found by: 756 mm Hg 41 mm Hg = 715 mm Hg 9 A The answer may be found using the combined gas law Removing the constant pressure leaves Charles s law: V1/T1 = V2/T2 This is rearranged to: T2 = V2T1/V1 = (2000 L 400 K)/ (800 L) = 1000 K (= 727 C) The other answers result from common errors in this problem 10 A The average kinetic energy of the molecules depends on the temperature The correct answer involves a temperature difference (333 K 303 K) Do not forget that ALL gas law calculations require Kelvin temperatures 11 A You can begin by removing the volume (constant) from the combined gas law to produce Gay-Lussac s law = P1/T1 = P2/T2.

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This equation may be rearranged to: P2 = P1T2/T1 = (0300 atm 290 K)/(300 K) = 0290 atm The moles are not important since they do not change Some of the other answers result from common errors 12 B The molar mass may be obtained by dividing the grams by the number of moles (calculated from the ideal gas equation) Do not forget to convert the temperature to kelvin 13 C Choice I requires an increase in volume Choice II requires an increase in temperature Choice III requires a change in the composition of the gas 14 B Lighter gases effuse faster The only gas among the choices that is lighter than methane is helium To calculate the molar mass, you would begin with the molar mass of methane and divide by the rate difference squared: M A = M B ( 1 2 )2 15.

D A steel tank will have a constant volume, and the problem states that the temperature is constant Adding gas to the tank will increase the number of moles (molecules) of the gas and the pressure (forcing the molecules closer together) A constant temperature means there will be a constant average speed 16 B The pressure is calculated using the ideal gas equation A common mistake is forgetting that 5 mol of gas are produced for every 2 mol of solid reactant The ideal gas equation is rearranged to P = nRT/V = (5 2)(02 mol) 1 1 (0082 L atm mol K ) (300 K)/(2 L) = 6 atm 17 E The lighter the gas, the faster it effuses (escapes) Equal moles of gases in the same container would give equal initial partial pressures.

The partial pressures would be reduced relative to the masses of the molecules, with the lightest gas being reduced the most 18 C Deviations from ideal behavior depend on the size and the intermolecular forces between the molecules The greatest deviation would be for a large polar molecule Sulfur tetrafluoride is the largest molecule, and it is the only polar molecule listed 19 D The molar mass of gas must be determined The simplest method to find the molar mass is: (547 g/L) (224 L/mol) = 123 g/mol (simple factor label) The molar mass may also be determined by dividing the mass of the gas by the moles (using 224 L/mol for a gas at STP and using 1 L) If you did not recognize the conditions as STP, you could find the moles from the ideal gas equation.

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