The production of ammonia from nitrogen and hydrogen under a given set of condit

Question

The production of ammonia from nitrogen and hydrogen under a given set of conditions is: N2 + 3 H2 (g) --> 2 NH3 (g)

(a) Suppose in one experiment, the concentration of ammonia increases from 0.257 M to 0.815 M in 15.0 min. What is the average rate of the reaction over this time interval?

(b) What is the change in concentration of N2 for that same time period?

(c) Suppose the rate law for this reaction is 1st order with respect to N2 and 2nd order with respect to H2. What is the rate constant and units for the reaction if the initial rate of the reaction is 0.15 mol/L min when [N2] = 0.10 M and [H2] = 0.20 M?

Explanation / Answer

a) average rate=(change in concentration÷time taken)/2=((0.815-0.257)÷15)÷2=1.86×10-2M.min-1

b) rate of change in concentration of N2= average rate

so change in concentration= 1.82×102×15=0.273M

C) rate=k[N2][H2]2

K=( 0.15)÷(0.10×0.20×0.20)=37.5M-2S-1

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