Which mechanism for species A reacting to form species D matches the graph? (A)

Question

Which mechanism for species A reacting to form species D matches the graph? (A) A rightarrow B fast step B rightarrow C slow step C rightarrow D fast step (B) A rightarrow B slow step B rightarrow C fast step C rightarrow D fast step (C) A rightarrow B slow step B rightarrow C fast step C rightarrow D slow step (D) A rightarrow B slow step B rightarrow D fast step Consider this reaction. 2 NO_2 (g) + F_2 (g) rightarrow 2NO_2] [F_2] Which mechanism is consistent with the rate law? (A) 2NO_2 (g) + F_2 (g) rightarrow 2NO_2 F(g) (B) NO_2 (g) + F_2 (g) rightarrow NO_2 (g) + Fe_(g) (C) F_2 (g) rightarrow 2F(g) 2NO_2 (g) + 2F(g) rightarrow 2NO_2 F(g) (D) NO_2 (g) + F_2 (g) rightarrow 2NO_2 F(g) (D) NO_2 (g) + F_2 (g) rightarrow NO_2 F(g) + F(g) NO_2 (g) + F(g) rightarrow NO_2 F(g) The decomposition of hydrogen peroxide is described by the equation 2H_2 O_2 (aq) rightarrow 2H_2 O (l) + O_2 (g) The reaction is first order in H_2 O_2. It takes 10.0 hours for the concentration of H_2 O_2 to drop from 0.500 M to 0.250 M. How many hours are required for the 0.250 M. How many hours are required for the concentration of H_2 O_2 to drop from 0.400 M to 0.100 M? (A) 38.0 h (B) 24.0 h (C) 20.0 h (D) 12.0 h Consider the first order reaction A rightarrow B, where A rearranges to give B. How many particles of A exist at t = 2 min? (A) 0 (B) 2 (C) 4 (D) 8 If a reaction is exothermic and is accompanied by a decrease in entropy of the system, then the reaction is (A) spontaneous at low temperatures only. (B) spontaneous at high temperatures only. (C) spontaneous at all temperatures. (D) nonspontaneous at all temperatures. What is the Gibbs Free Energy change for the reaction C_3 H_8 (g) + 5O_2 (g) rightarrow 3CO_2 (g) + 4H_2 O(l) (A) -2111 kJ (B) + 2111 kJ (C) -108.932 kJ (D) +108.932 kJ For which should Delta H degree and Delta G degree be about equal? (A) 2NO_2 (g) rightarrow N_2 O_4 (g) (B) 2H_2 (g) + O_2 (g) rightarrow 2H_2 O(g) (C) 2Al (s) + Fe_2 O_3 (s) rightarrow 2Fe_(s) + Al_2 O_3 (s) (D) 2Na_(z) + 2H_2 O_(l) rightarrow 2NaOH(aq) + H_2 (g) What is the entropy change for this reaction? C_3 H_8 (g) + 5O_2 (g) rightarrow 3CO_2 (g) + 4H_2 O(l) (A) -191 J middot K^-1 (B) -373 J middot K^-1 (C) +373 J middot K^-1 (D) -191 J middot K^-1

Explanation / Answer

7)

Answer A

Activation energy of B—>C is largest. So, it is slowest

The step with largest activation energy will always be slowest

8)

Answer: D

Rate depends on the slowest step

in D slowest step is 1st step

So, rate law for D will be:

rate = k [NO2][F2]

I am allowed to answer only 1 question at a time

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