Question

For the decomposition of ammonia on a platinum surface at 856 °C

Answer 1

$\\ \tt\leadsto \dfrac{d[NH_3]}{dt}=1.50\times 10^{-6}$

• dt remains same for reaction

$\\ \tt\leadsto \dfrac{d[H_2]}{dt}=\dfrac{3}{2}\dfrac{d[NH_3]}{dt}$

$\\ \tt\leadsto \dfrac{d[H_2]}{dt}=\dfrac{3}{2}(1.5\times 10^{-6})$

$\\ \tt\leadsto \dfrac{d[H_2]}{dt}=2.25\times 10^{-6}Ms^{-1}$

M is molarity here not metre