Consider the following reactionN2(g)+3H2(g)→2NH3(g) . The rate of the reaction in terms of N2 at T (k) is−d[N2]dt=0.02 mole.lit−1.sec−1 . What is the value of −d[H2]dt(in mole.lit−1.sec−1) at the same temperature?

Rate =−d[N2]dt=13[−dH2dt] −d[H2]dt=3[−d[H2]dt] =3×0.02 =0.06 M.sec−1

Consider the following reactionN2(g)+3H2(g)→2NH3(g) . The rate of the reaction in terms of N2 at T (k) is−d[N2]dt=0.02 mole.lit−1.sec−1 . What is the value of −d[H2]dt(in mole.lit−1.sec−1) at the same temperature?

Rate =−d[N2]dt=13[−dH2dt] −d[H2]dt=3[−d[H2]dt] =3×0.02 =0.06 M.sec−1

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Consider the following reaction $N_{2 (g)} + 3 H_{2 (g)} \to 2 N H_{3 (g)}$ . The rate of the reaction in terms of $N_{2}$ at T (k) is $- \frac{d [N_{2}]}{d t} = 0.02 m o l e . l i t^{- 1} . \sec^{- 1}$ . What is the value of $- \frac{d [H_{2}]}{d t} (i n m o l e . l i t^{- 1} . \sec^{- 1})$ at the same temperature?

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$0.04$

$50$

$0.06$

$0.02$

answer is C.

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Detailed Solution

$Rate = - \frac{d [N_{2}]}{d t} = \frac{1}{3} [\frac{- d H_{2}}{d t}]$

$- \frac{d [H_{2}]}{d t} = 3 [\frac{- d [H_{2}]}{d t}]$

$= 3 \times 0.02$

$= 0.06 M . \sec^{- 1}$

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Consider the following reactionN2(g)+3H2(g)→2NH3(g) . The rate of the reaction in terms of N2 at T (k) is−d[N2]dt=0.02 mole.lit−1.sec−1 . What is the value of −d[H2]dt(in mole.lit−1.sec−1) at the same temperature?

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