Question 41 : A catalyst increases the rate of a reaction by:
1. increasing the temperature.
2. decreasing the activation energy.
3. increasing the activation energy.
4. decreasing the temperature.
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Question 42 : Which of the following are catalysts:
1. Br₂
2. OBr₂
3. H₂O
4. Both Br₂ and OBr₂ are catalysts.
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Question 43 : Reaction rates increase with temperature because as the temperature increases:
1. the activation energy increases
2. the activation energy decreases.
3. the equilibrium constant increases.
4. the rate constant increases.
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Question 44 : For the following reaction DG° is 60 kJ/mole at 25° C. The equilibrium constant for this reaction at 25° C is: H2 (g) + I2 (g) « 2HI (g)
1. 0.35
2. 86
3. 0.999
4. 05 x 10^-3
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Question 45 : Which of the following are reaction intermediates:
1. H₂O
2. Br^-
3. None are reaction intermediates
4. OBr^-
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Question 46 : You would expect the half-life of phosphine at room temperature to be _____ than at 680° C.
1. longer
2. shorter
3. Not enough information given. Must know DH to answer this.
4. the same
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Question 47 : The rate law for this reaction is:
1. Rate = k[H₂O₂][OBr^-]
2. Rate = k[H₂O₂]₂ [Br^- ]
3. Rate = k[H₂O₂]₂
4. Rate = k[H₂O₂][Br^-]
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Question 48 : What is the half-life of phosphine (problem 14) at 680° C?
1. 35 s
2. 0.029 s
3. 0.014 s
4. 55 s
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Question 49 : The following reaction is found to be first order in H2 (g) and second order in NO (g). The rate law for this reaction is: 2NO (g) + 2H2-> N2 (g) + 2H₂O (g)
1. Rate = k[NO][H₂]₂
2. Rate = k[NO]2[H2]2/[N2][H₂O]₂
3. Rate = k[NO]₂[H₂]₂
4. Rate = k[NO]₂[H₂]
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Question 50 : A catalyst functions by:
1. providing a reaction path with a lower activation energy
2. lowering the energy of the reactants.
3. lowering the energy of the products.
4. increasing the equilibrium constant.
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