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?

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