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1 February, 18:05

Given the following reaction: 2D (g) + 3E (g) + F (g) ⟶ 4G (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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  1. 1 February, 18:10
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    1) The concentration of H is increasing, half as fast as D decreases: 0.05 mol L-1. s-1

    2) The concentration of E decreseas 3/4 as fast as G increases = 0.15 mol L-1. s-1

    3) Reaction rate = - (Δ[D]) / (2Δt) = - (Δ[E]) / (3Δt) = - (Δ[F]) / (Δt) = (Δ[G]) / (4Δt) = (Δ[H]) / (Δt)

    Explanation:

    ⇒The equation

    2D (g) + 3E (g) + F (g) ⟶ 4G (g) + H (g)

    The reaction rate will be expressed like:

    Reaction rate = - (Δ[D]) / (2Δt) = - (Δ[E]) / (3Δt) = - (Δ[F]) / (Δt) = (Δ[G]) / (4Δt) = (Δ[H]) / (Δt)

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

    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

    E decreseas 3/4 as fast as G increases = 0.15 mol L-1. s-1
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