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Question: In a catalytic conversion of \(N_{2}\) to \(NH_{3}\) by Haber's process, the rate of reaction was ex...

In a catalytic conversion of N2N_{2} to NH3NH_{3} by Haber's process, the rate of reaction was expressed as change in the concentration of ammonia per time is

40×10−3mollitre−1s−140 \times 10^{- 3}mollitre^{- 1}s^{- 1}. If there are no side reaction, the rate of the reaction as expressed in terms of hydrogen is (in mol litre−1s−1litre^{- 1}s^{- 1})

A

60×10−360 \times 10^{- 3}

B

20×10−320 \times 10^{- 3}

C

1.200

D

10.3×10−310.3 \times 10^{- 3}

Answer

60×10−360 \times 10^{- 3}

Explanation

Solution

−d(N2)dt=−13d(H2)dt=12d(NH3)dt\frac{- d(N_{2})}{dt} = - \frac{1}{3}\frac{d(H_{2})}{dt} = \frac{1}{2}\frac{d(NH_{3})}{dt}=32×40×10−3\frac{3}{2} \times 40 \times 10^{- 3}

=60×10−3.= 60 \times 10^{- 3}.