Explanation:
Rate constant = 6.08 x 10–4 s–1
What is the rate of the reaction when [N2O5] = 0.100 M..?
A first-order reaction depends on the concentration of one reactant, and the rate law is:
r= −dA / dt = k[A]
Rate of reaction = k [ A ]
where [A] = 0.100 M
Rate of reaction = (6.08 x 10–4) x 0.100
Rate of reaction = 6.08 x 10–5 Ms–1
what happens to the rate when the concentration of N2O5 is doubled to 0.200 M?
Rate of reaction = k [ A ]
[A] = 0.200
Rate of reaction = (6.08 x 10–4) x 0.200
Rate of reaction = 1.216 x 10–4 Ms–1
The rate of the reaction increases to 1.216 x 10–4 Ms–1
