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

i'm wiling to try and you : )

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8