Solution Found!
Answer: Consider the following reaction, which takes place
Chapter 14, Problem 36P(choose chapter or problem)
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 \(k_{f}\).
Questions & Answers
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.