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The reaction 2NO(g) + H(2)(g) to N(2)O(g...

The reaction `2NO(g) + H_(2)(g) to N_(2)O(g) + H_(2)O(g)` follows the rate law `(dp(N_(2)O))/(dt)= k(p_(NO))^(2)p_(H_(2))`. If the reaction is initiated with `p_(NO)= 1000` mm Hg and `p_(H_(2))`=10mm Hg. The reaction may be considered to follow:

A

first order kinetics

B

second order kinetics

C

zero order kinetics

D

third order kinetics

Text Solution

Verified by Experts

The correct Answer is:
A
Here `p_(NO) gt gt p_(H_(2))` Hence the given rate reaction can be approximate as `(dp_(N_(2)O))/(dt)=kp_(H_(2))` where `k=k(P_(NO))^(2)`
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