Question #184190

Decomposition of a N_{2}O_{5} solution in water takes place via the following reaction:

2 N_{2}O_{5} → 4 NO_{2} + O_{2}

A scientist obtained some experimental data comparing the rate of decomposition and [N_{2}O_{5}]:

**[N**_{2}**O**_{5}**]**0.45 M, 0.90 M

**Rate**2.7 x 10^{-4} M/s , 5.4 x 10^{-4} M/s

Assuming that the rate law is in the following form:

Rate = k[N_{2}O_{5}]^{a}

Determine the value of “a”.

**Part B**

Calculate “k”.

**Part C**

Calculate the rate of reaction when the concentration of N_{2}O_{5} is 0.014 M.

Expert's answer

Part A: 4

Part B: 2

"Part C: 8.4\u00d710^-6"

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