Given the following reaction: 2D (g) + 3E (g) + F (g) / longrightarrow⟶ 2G (g) + H (g) When the concentration of D is decreasing by 0.10 M/s, how fast is the concentration of H increasing? When the concentration of G is increasing by 0.20 M/s, how fast is the concentration of E decreasing? What is the rate of reaction?

Question

Chemistry

Ignacio Curtis

3 September, 18:51

Given the following reaction: 2D (g) + 3E (g) + F (g) / longrightarrow⟶ 2G (g) + H (g) When the concentration of D is decreasing by 0.10 M/s, how fast is the concentration of H increasing? When the concentration of G is increasing by 0.20 M/s, how fast is the concentration of E decreasing? What is the rate of reaction?

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Answers (1)

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Aldo Glenn · Answer 1

Rate of reaction = - d[D] / 2dt = - d[E] / 3dt = - d[F]/dt = d[G]/2dt = d[H]/dt

The concentration of H is increasing, half as fast as D decreases: 0.05 mol L-1. s-1

E decreseas 3/2 as fast as G increases = 0.30 M/s

Explanation:

Rate of reaction = - d[D] / 2dt = - d[E] / 3dt = - d[F]/dt = d[G]/2dt = d[H]/dt

When the concentration of D is decreasing by 0.10 M/s, how fast is the concentration of H increasing:

Given data = d[D]/dt = 0.10 M/s

-d[D] / 2dt = d[H]/dt

d[H]/dt = 0.05 M/s

The concentration of H is increasing, half as fast as D decreases: 0.05 mol L-1. s-1

When the concentration of G is increasing by 0.20 M/s, how fast is the concentration of E decreasing:

d[G] / 2dt = - d[H]/3dt

E decreseas 3/2 as fast as G increases = 0.30 M/s