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Answer: Consider the following reaction, which takes place

Chapter 14, Problem 36P

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QUESTION:

Consider the following reaction, which takes place in a single elementary step:

\(2A+B\ \xrightarrow[{k_{-1}}]{{k_{1}}}\ A_{2}B\)

If the equilibrium constant \(K_{c}\) is 12.6 at a certain temperature and if \(k_{T}=5.1 \times 10^{-2}\ \mathrm{s}^{-1}\), calculate the value of \(k_{f}\).

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QUESTION:

Consider the following reaction, which takes place in a single elementary step:

\(2A+B\ \xrightarrow[{k_{-1}}]{{k_{1}}}\ A_{2}B\)

If the equilibrium constant \(K_{c}\) is 12.6 at a certain temperature and if \(k_{T}=5.1 \times 10^{-2}\ \mathrm{s}^{-1}\), calculate the value of \(k_{f}\).

ANSWER:

Step 1 of 3

Equilibrium constant can be expressed as the ratio of forward constant to the rate of backward rate constant for the reverse reaction. It is a constant for specific reactions at specific temperatures.

It can be expressed as follows;

                                                                ........................(1)

 and  are the rate constants.

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