The rate law for the mechanism below is
A2(g) ⇌
2A(g) K1, fast
A(g) + B(g) ⇌
AB(g) K2, fast
AB(g) + A(g) →
A2B(g) k3,
slow
Options:
rate = K2k3[A]2[B] |
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rate = K1K2k3 [A2][B] |
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rate = K10.5k3 [A2]0.5[AB] |
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rate = k3[A][AB] |
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rate = K10.5K2k3 [A2]0.5[A] [B] |
Rate of reaction is determined by slowest step of the reaction
As in the question third step is the slowest step
rate =k3 [A][AB]
The rate law for the mechanism below is A2(g) ⇌ 2A(g) K1, fast A(g) + B(g) ⇌...
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