A possible mechanism for a reaction that takes place in solution is Step(l): Ce^

Question

A possible mechanism for a reaction that takes place in solution is Step(l): Ce^4+ + Mn^2+ --- rightarrow Ce^3+ + Mn^3+ slow Step (2) Ce^4+ + Mn^3+ --- rightarrow Ce^3+ + Mn^4+ fast Step (3): Mn^4+ + Tl^1+ ---- rightarrow Mn^2+ + Tl^3+ fast What is the for the overall reaction what is the predicted rate law which species is (are) intermediates, and which species is the catalyst? A sample of N_2O_4 (0.400 mol) was placed in an empty 1.00 L container at 500 K. After equilibrium was reached, the concentration of NO_2 was found to be 6.29 times 10^-4 M. Calculate the value of k_c at 500 K for the reaction: N_2O_4(g) Equilibrium 2 NO_2(g)

Explanation / Answer

Ce+4 + Mn+2 = Ce+3 + Mn+3

Ce+4 + Mn+3 = Ce+3 + Mn+4

Mn+4 + Tl+1 = Mn+2 + Tl+3

a)

overall reaction

Ce+4 + Mn+2 + Ce+4 + Mn+3 +Mn+4 + Tl+1 = Ce+3 + Mn+3+Ce+3 + Mn+4+Mn+2 + Tl+3

cancel common terms:

2Ce+4 + Tl+1 = 2Ce+3 + Tl+3

b)

predicted rate law... will be that of the slow reaction:

Rate = k[Ce+4][Mn+2]

c)

from this, find intermediates:

Ce+4 + Mn+2 + Ce+4 + Mn+3 +Mn+4 + Tl+1 = Ce+3 + Mn+3+Ce+3 + Mn+4+Mn+2 + Tl+3

the intermediates are shown in bold letters

Mn+2, Mn+3, Mn+4

d)

catalys --> Manganese is the catalyst since it provides +2,+3,+4 electron flow

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