Question

For the first-order decomposition of N₂O₅ (g) written as

2 N₂O₅ (g) ¾® 4 NO₂ (g) + O₂ (g) rate= K [N₂O₅]

N₂O₅ (g) ¾® 2 NO₂ (g) + $\frac{1}{2}$O₂ (g) rate = K^¢[N₂O₅]

Which of the following relation is correct?

• A. K = K¢
• B. K > K¢
• C. K > 2K¢
• D. 2K = K¢

Answer 1

Answer: (D)

2K = K¢

Answer 2

The rate of reaction as per first equation is

–$\frac{1}{2}$ $\frac{d\lbrack N_{2}O_{5}\rbrack}{dt}$ = K [N₂O₅]

or $\frac{- d\lbrack N_{2}O_{5}\rbrack}{dt}$ = 2K [N₂O₅]

As per second reaction the rate of reaction is

$\frac{- d\lbrack N_{2}O_{5}\rbrack}{dt}$ = K^¢ [N₂O₅]

\ 2K = K¢