Question

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?

Answer 1

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)

Step-by-step 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