Question

The reaction NO2(g) + CO(g) → NO(g) + CO2(g) has been found to be second order with respect to NO2 and zero order with respect to CO. At a certain temperature, the rate constant is found experimentally to be 3.0 × 10−5 L mol · s . What is the rate of formation

Answer 1

Answer:

The answer is " $122.88 \times 10^{-5}$"

Explanation:

In the given question some data is missing. so, the correct solution can be defined as follows:

Missing values:

$k= 3.0 \times 10^{-5}\\\\NO_2 =6.4 \ mol / l \\\\CO= 4.1 mol / l \\\\NO= 5.2 mol / l \\\\CO_2= 1.3 mol / l$

Given equation:

$NO_2(g) + CO(g) \longrightarrow NO(g) + CO_2(g)$

In the above equation, the rate is $=k.[NO_2]^2$ because the above given is the part of the second-order, which relates to $NO_2$. In the zeros order the Carbon monoxide (CO) its reaction doesn't affect the rate.

Calculating the rate:

Rate $=k.[NO_2]^2$

        $= 3.0 \times 10^{-5} \times 6.4^2\\\\=3.0 \times 10^{-5} \times 40.96\\\\= 122.88 \times 10^{-5}$