Question

# $$N_2(g)+3H_2(g)\rightarrow 2NH_3(g)$$ For the given reaction, under certain condition of temperature and partial pressure of the reactants, the rate of formation of $$NH_3$$ is $$10^{-3}\ kg hr^{-1}$$. The rate of conversion of $$H_2$$ under the same condition is:

A
1.5×103kghr1
B
1.76×104kghr1
C
2×103kghr1
D
3×103kghr1

Solution

## The correct option is B $$1.76\times 10^{-4} kg hr^{-1}$$$$\displaystyle N_2(g)+3H_2(g)\rightarrow 2NH_3(g)$$$$\displaystyle - \frac {1}{3} \frac {d}{dt} [H_2] = \frac {1}{2} \frac {d}{dt}[NH_3]$$$$\displaystyle - \frac {d}{dt} [H_2] = \frac {3}{2} \frac {d}{dt}[NH_3]$$The rate of formation of ammonia is $$10^{−3}$$ kg/hr. The rate of conversion of hydrogen under same condition is $$\displaystyle - \frac {d}{dt} [H_2] = \displaystyle \frac {3\times 2}{2\times 17} \times 10^{−3}$$ kg/hr $$= 1.76\times 10^{-4} \ kg hr^{-1}$$Hence, the correct option is $$A$$ChemistryNCERTStandard XII

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