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For the reaction $2H_{2}(g)+2NO(g)\rightarrow N_{2}(g)+2H_{2}O(g)$ the observed rate experssion is, rate $=k_{f}\left [ NO \right ]^{2}[H_{2}]$ . The rate expression for reverse reaction is:
Option: 1 $k_{b}[N_{2}][H_{2}O]^{2}$
Option: 2 $k_{b}[N_{2}][H_{2}O]$
Option: 3 $k_{b}[N_{2}][H_{2}O]^{2}/[H_{2}]$
Option: 4 $k_{b}[N_{2}][H_{2}O]^{2}/[NO]$

Answers (1)

best_answer

Therefore, Option(3) is correct.

Posted by

Kuldeep Maurya

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