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Q.

For the reaction : $N_{2} (g) + 3 H_{2} (g) ⟶ 2 {NH}_{3} (g)$ . If rate of appearance of ${NH}_{3}$ is $6.8 \times 10^{- 3} gm / \min,$ then rate of disappearance of $H_{2} (g)$ at the same condition will be

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a

$6 \times 10^{- 4} gm / \min$

b

$1.02 \times 10^{- 2} gm / \min$

c

$6.8 \times 10^{- 3} gm / \min$

d

$1.2 \times 10^{- 3} gm / \min$

answer is D.

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Detailed Solution

The rate of disappearance of $H_{2} (g)$ ,

$\frac{- d [H_{2}]}{dt} = \frac{1}{2} \frac{d [{NH}_{3}]}{dt}$

$= \frac{1}{2} \times \frac{6.8 \times 10^{- 8}}{17} \times 2 \times 3 = 1.2 \times 10^{- 3} gm / \min$

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For the reaction : N2(g)+3H2(g)⟶2NH3(g). If rate of appearance of NH3 is 6.8×10−3gm/min, then rate of disappearance of H2(g) at the same condition will be