The mechanism of the reaction,$2NO_{(g)} + 2H_{2(g)} \to N_{2(g)} + 2H_2O_{(g)}$ is:
Step $1$: $2NO_{(g)} + H_{2(g)} \xrightarrow{\text{slow}} N_2 + H_2O_2$
Step $2$: $H_2O_2 + H_2 \xrightarrow{\text{fast}} 2H_2O$
Then the correct statement is:

• A
  Rate $= k [NO]^2 [H_2]$
• B
  Rate $= k [H_2O_2] [H_2]$
• C
  On doubling the concentration of $H_2$,keeping the concentration of $NO$ constant,the rate will become double
• D
  If the initial concentration of $H_2$ and $NO$ is $C_0$ and after time $t$ the concentration of $N_2$ is $x$,then Rate $= k (C_0 - 2x)^2$