The rate constant,$k$,of a zero order reaction $2 NH_3(g) \xrightarrow[1130 \ K]{Pt} N_2(g) + 3 H_2(g)$ is $y \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of hydrogen (in $mol \ L^{-1} \ s^{-1}$) is
- A$y \times 10^{-4}$
- B$2 y \times 10^{-4}$
- C$3 y \times 10^{-4}$
- D$\frac{y}{3} \times 10^{-4}$
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