We read your photo as:

1 the rate of reaction 2 the half life

July 6, 2026Chemistry

ScanSolve AI Answer

Answer

\text{2.0} \times 10^{-5} \text{ mol dm}^{-3}\text{ s}^{-1}

\text{346.5 s}

3 steps

Here's how to solve this problem:

Identify the given information.
The reaction is first order.
The concentration of the reactant, $[\text{N}_2\text{O}_5] = 0.01 \text{ mol/dm}^3$ .
The specific rate constant, $k = 2.0 \times 10^{-3} \text{ s}^{-1}$ .
Calculate the rate of reaction.
For a first-order reaction, the rate law is:
$\text{Rate} = k[\text{N}_2\text{O}_5]$
Substitute the given values:
$\text{Rate} = (2.0 \times 10^{-3} \text{ s}^{-1}) \times (0.01 \text{ mol/dm}^3)$ $\text{Rate} = 2.0 \times 10^{-5} \text{ mol dm}^{-3}\text{ s}^{-1}$
The rate of reaction is $\boxed{\text{2.0} \times 10^{-5} \text{ mol dm}^{-3}\text{ s}^{-1}}$ .
Calculate the half-life.
For a first-order reaction, the half-life ( $t_{1/2}$ ) is given by the formula:
$t_{1/2} = \frac{0.693}{k}$
Substitute the value of $k$ :
$t_{1/2} = \frac{0.693}{2.0 \times 10^{-3} \text{ s}^{-1}}$ $t_{1/2} = 346.5 \text{ s}$
The half-life is $\boxed{\text{346.5 s}}$ .

Was this helpful?

A new problem that tests the same skill.

Ask a follow-up, and the answer starts from this question.

Got a different question?Ask your own question

Handwritten Step-by-Step Solution

Get this as a handwritten image on WhatsApp — like a tutor wrote it for you.