The compound AX2 decomposes according to the equation, 2 AX2 (g) = > 2 AX (g) + X2 (g). In one experiment, AX2 was measured at various times, and these data recorded: Time (s) AX2 mol/L 0 0.0500 2.0 0.0448 6.0 0.0300 8.0 0.0249 10.0 0.0209 20.0 0.0088 What is the average rate from 6.0 to 10.0 seconds in mol / L s? Use 4 decimal places.

Question

Chemistry

Ramon

5 October, 05:47

The compound AX2 decomposes according to the equation, 2 AX2 (g) = > 2 AX (g) + X2 (g). In one experiment, AX2 was measured at various times, and these data recorded: Time (s) AX2 mol/L 0 0.0500 2.0 0.0448 6.0 0.0300 8.0 0.0249 10.0 0.0209 20.0 0.0088 What is the average rate from 6.0 to 10.0 seconds in mol / L s? Use 4 decimal places.

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Mike Summers · Answer 1

0.0011 mol/L. s

Explanation:

The average rate of disappearing of the reagent is the variation of the concentration of it divided by the time that this variation is being measured. The reaction rate, is proportional to the coefficient of the substance, so, for a generic reaction:

aA + bB - -> cC + dD

rate = - (1/a) Δ[A]/Δt = - (1/b) Δ[B]/Δt = (1/c) Δ[C]/Δdt = (1/d) Δ[D]/dt

The minus sign is because of the reagent is desapering, so:

rate = - (1/2) * (0.0209 - 0.0300) / (10 - 6)

rate = 0.0011 mol/L. s