In a catalytic conversion of N2 to NH3 by Haber s process, the rate of reaction expressed as change in the concentration of ammonia per unit time is 40 × 10-3 mole L-1 s-1. If there are no side reactions, the rate of the reaction expressed in terms of hydrogen is

Question

In a catalytic conversion of N2 to NH3 by Haber s process, the rate of reaction expressed as change in the concentration of ammonia per unit time is 40 × 10-3 mole L-1 s-1. If there are no side reactions, the rate of the reaction expressed in terms of hydrogen is (A) 60 × 10-3 mol L -1 s -1 (B) 20 × 10-3 mol L -1 s -1 (C) 1200 mol L -1 s -1 (D) 10.3 × 10-3 mol L -1 s -1

Tardigrade Admin · Accepted Answer

N 2+3 H 2 arrow 2 NH 3 Rate =(1/3) (d[ H 2]/d t)=(1/2) (d[ NH 3]/d t) ⇒ (d[ H 2]/d t)=(3/2) 40 × 10-3 =60 × 10-3 mol L -1 s -1

Q. In a catalytic conversion of $N_{2}$ to $N H_{3}$ by Haber s process, the rate of reaction expressed as change in the concentration of ammonia per unit time is $40 \times 1 0^{- 3}$ mole $L^{- 1} s^{- 1.}$ If there are no side reactions, the rate of the reaction expressed in terms of hydrogen is

$60 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

$20 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

$1200 m o l L^{- 1} s^{- 1}$

$10.3 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

$N_{2} + 3 H_{2} \to 2 N H_{3}$
Rate $= \frac{1}{3} \frac{d [ H _{2} ]}{d t} = \frac{1}{2} \frac{d [ N H _{3} ]}{d t}$
$\Rightarrow \frac{d [ H _{2} ]}{d t} = \frac{3}{2} 40 \times 1 0^{- 3}$
$= 60 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

Q. In a catalytic conversion of N2​ to NH3​ by Haber s process, the rate of reaction expressed as change in the concentration of ammonia per unit time is 40×10−3 mole L−1s−1. If there are no side reactions, the rate of the reaction expressed in terms of hydrogen is

60×10−3molL−1s−1

20×10−3molL−1s−1

1200molL−1s−1

10.3×10−3molL−1s−1