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balandron [24]
3 years ago
14

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 t

o 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
Chemistry
1 answer:
hodyreva [135]3 years ago
7 0

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}\\

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Since we have 2B, multiply the whole of II. by 2:

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Reversing III. gives us a negative enthalpy change as such:

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Thus, the first option is the correct answer.

Supplementary:

To learn more about Hess's Law, do check out: brainly.com/question/26491956

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