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

Chemistry
NCERT
Standard XII

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