Chemistry

Chemistry

Problem

For the decomposition reaction 2 NO2(g)→2\,\text{NO}_2(g)\rightarrow products, the rate law is rate=k[NO2]2\text{rate}=k[\text{NO}_2]^2. When the initial concentration of NO2\text{NO}_2 is 0.025 M0.025\,\text{M}, the initial rate is measured to be 3.2×10−4 M s−13.2\times10^{-4}\,\text{M}\,\text{s}^{-1}. What is the value of the rate constant kk? a) 2.56×10−1 M−1 s−12.56\times10^{-1}\,\text{M}^{-1}\,\text{s}^{-1} b) 5.1×100 M−1 s−15.1\times10^{0}\,\text{M}^{-1}\,\text{s}^{-1} c) 5.1×10−1 M−1 s−15.1\times10^{-1}\,\text{M}^{-1}\,\text{s}^{-1} d) 5.1×10−3 M−1 s−15.1\times10^{-3}\,\text{M}^{-1}\,\text{s}^{-1}

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