Chemical Kinetics and Nuclear ChemistryMedium

Question

For the reaction N2(g) + 3H2(g) → 2NH3(g) under certain conditions of temperature and partial pressure of the reactants, the rate of formation of NH3 is 10−3 kg h−1. The rate of consumption of H2 under same condition is

Options

A.1.5 × 10−3 kg h−1
B.1.76 × 10−4 kg h−1
C.6.67 × 10−4 kg h−1
D.3 × 10−3 kg h−1

Solution

$\frac{r_{H_{2}}}{3} = \frac{r_{NH_{3}}}{2} \Rightarrow r_{H_{2}} = \frac{3}{2} \times \frac{10^{- 3}}{17} \times 10^{- 3}\text{ mol h}\text{r}^{- 1}$

$= \frac{3}{34} \times \frac{2}{10^{3}}\text{ Kg h}\text{r}^{- 1} = 1.76 \times 10^{- 4}\text{ Kg h}\text{r}^{- 1}$

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