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## Question:

The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Starting with 8.00×10−2 mol of N2O5(g) in a volume of 2.9 L, how many moles of reactant are left after 5 minutes? What is its half-life?

## Answer:

**Answer:**

0.01034 moles of reactant are left after 5 minutes.

101.63 sec is the half-life.

**Explanation:**

Using integrated rate law for first order kinetics as:

Where,

is the concentration at time t

is the initial concentration = mol

k is the rate constant = s⁻¹

Time = 5 minutes = 5*60 seconds = 300 seconds ( 1 min = 60 sec)

Thus,

**0.01034 moles of reactant are left after 5 minutes.**

Given that:

k = s⁻¹

The expression for half life is:-

**101.63 sec is the half-life.**

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