This graph shows the concentration of the reactant a in the reaction a→b.

determine the average rate of the reaction between 0 and 10 seconds.

0.007 m/s
0.014 m/s
0.86 m/s
0.07 m/s

0.014 M/s

Explanation:

The rate of a reaction depends on the concentration of a particular compound and it stoichmetry coefficient. For the reaction:

aA + bB → cC +dD

The rate can be calculated:

r = -(1/a)xΔ[A]/Δt = -(1/b)xΔ[B]/Δt = (1/c)xΔ[C]/Δt = (1/d)xΔD/Δt

The minus signal for the reagents its because they are being consumed, so Δ[A] and Δ[B] will be negative, and r must be positive. Δt is the time variation.

So, for the reaction given, in t = 0, [A] =1 M, and in t= 10s, [A] = 0.86 M, then

Δ[A] = -0.14 M

r = -(Δ[A]/Δt)

r = -(-0.14/10)

r = 0.014 M/s

just did the assignment and the answer was #1 +2 n