8. Ammonia is formed from the reaction as follows: N2 (g) + 3 H2 (g) ----> 2 NH3

Question

8. Ammonia is formed from the reaction as follows: N2 (g) + 3 H2 (g) ----> 2 NH3( g )Determine (a) the order of each reactant, (b) the order of the reaction, (c) write the rate law and (d) calculate the rate constant k, for the following data:   
Reaction / [N2]o / [H2]o / initial rate
1. 0.20 M / 0.10 M / 3.50 × 10-3 M/s

2. 0.40 M / 0.10 M / 7.00 × 10-3 M/s

3. 0.40 M / 0.40 M / 7.00 × 10-3 M/s

Can someone explain to me how to solve this chemistry problem? The answers are shown below

Answers: (a) 1st order N2 and zero order H2; (b) overall order 1st order; (c) rate = k[N2]; (d) k = 0.0175 s-1.

Explanation / Answer

a)
see reaction 1 and 2
[N2] becomes 0.40/0.20 = 2 times
[H2] doesn't chnage
rate becomes (7.00*10^-3)/(3.50*10^-3)= 2 times
so, order of N2 is 1

see reaction 2 and 3
[N2] doesn't chnage
[H2] becomes 0.40/0.10 = 4 times
rate doesn't chnage
so, order of H2 is 0

b)
order of reaction = sum of order of each reactant
= 1+0
= 1

c)
rate law is:
rate = k [N2]

D)
rate = k [N2]
put value for reaction 1
3.50*10^-3 M/s = k (0.20)
k = 0.0175 s-1

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