For N2+3H2⟶2NH3, rates of disappearance of N2 and H2 and rate of appearance of NH3respectively are a, b and c, then

For the given reaction,Rate=-ddt N2=-13ddtH2=+12ddtNH3∴a < c < b

For N2+3H2⟶2NH3, rates of disappearance of N2 and H2 and rate of appearance of NH3respectively are a, b and c, then

For the given reaction,Rate=-ddt N2=-13ddtH2=+12ddtNH3∴a < c < b

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For $N_{2} + 3 H_{2} ⟶ 2 {NH}_{3}$ , rates of disappearance of N₂ and H₂ and rate of appearance of NH₃
respectively are a, b and c, then

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a > b > c

a < c < b

a = b > c

a = b = c

answer is B.

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Detailed Solution

For the given reaction,

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

$∴$ a < c < b

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For N2+3H2⟶2NH3, rates of disappearance of N2 and H2 and rate of appearance of NH3respectively are a, b and c, then

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For $N_{2} + 3 H_{2} ⟶ 2 {NH}_{3}$ , rates of disappearance of N₂ and H₂ and rate of appearance of NH₃
respectively are a, b and c, then