Questions: The reaction A=B was run with an initial concentration of 0.26 M . Determine the equilibrium concentration (in M ) of B given that the rate constant is 7,018 . REPORT YOUR ANSWER TO 2 DECIMAL PLACES. DO NOT INCLUDE UNITS.

Solution Steps

The reaction \( A \rightarrow B \) is given with an initial concentration of \( [A]_0 = 0.26 \) M. The rate constant \( k = 7018 \). We need to determine the equilibrium concentration of \( B \).

Since the rate constant is given, we assume this is a first-order reaction. The rate law for a first-order reaction is: \[ \frac{d[A]}{dt} = -k[A] \]

The integrated rate law for a first-order reaction is: \[ [A] = [A]_0 e^{-kt} \]

At equilibrium, the concentration of \( A \) will be very small, approaching zero, because the rate constant is very high. Thus, almost all \( A \) will have converted to \( B \).

Since \( A \) converts to \( B \) completely, the equilibrium concentration of \( B \) will be approximately equal to the initial concentration of \( A \): \[ [B]_{eq} \approx [A]_0 = 0.26 \]

Final Answer