Chemistry

Chemistry

Problem

The reaction A+2 B→\text{A}+2\,\text{B}\rightarrow products follows the rate law rate=k[A]1[B]2\text{rate}=k[\text{A}]^1[\text{B}]^2. Initial-rate data are collected in two trials under identical temperature conditions: Trial 1: [A]=0.10 M[\text{A}]=0.10\,\text{M}, [B]=0.20 M[\text{B}]=0.20\,\text{M}, rate =1.6×10−3 M s−1=1.6\times10^{-3}\,\text{M}\,\text{s}^{-1} Trial 2: [A]=0.15 M[\text{A}]=0.15\,\text{M}, [B]=0.25 M[\text{B}]=0.25\,\text{M}, rate =3.8×10−3 M s−1=3.8\times10^{-3}\,\text{M}\,\text{s}^{-1} Based on these data, what is the value of the rate constant kk? a) 8.0×10−1 M−2 s−18.0\times10^{-1}\,\text{M}^{-2}\,\text{s}^{-1} b) 1.1×10−1 M−2 s−11.1\times10^{-1}\,\text{M}^{-2}\,\text{s}^{-1} c) 4.0×10−1 M−2 s−14.0\times10^{-1}\,\text{M}^{-2}\,\text{s}^{-1} d) 4.0×10−2 M−2 s−14.0\times10^{-2}\,\text{M}^{-2}\,\text{s}^{-1}

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