Chemistry

Chemistry

Problem

Consider the reaction A+B→\text{A}+\text{B}\rightarrow products, which proceeds by the following mechanism. Step 1 A ++ B ⟶\longrightarrow C (slow) Step 2 C ⟶\longrightarrow products (fast) The rate constant for Step 1 is k=2.5×10−2 M−1 s−1k=2.5\times10^{-2}\,\text{M}^{-1}\,\text{s}^{-1}. What is the initial rate of the overall reaction when [A]=0.050 M[\text{A}]=0.050\,\text{M} and [B]=0.10 M[\text{B}]=0.10\,\text{M}? a) 2.5×10−4 M s−12.5\times10^{-4}\,\text{M}\,\text{s}^{-1} b) 2.5×10−3 M s−12.5\times10^{-3}\,\text{M}\,\text{s}^{-1} c) 1.3×10−4 M s−11.3\times10^{-4}\,\text{M}\,\text{s}^{-1} d) 1.25×10−5 M s−11.25\times10^{-5}\,\text{M}\,\text{s}^{-1}

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