Problem

Problem

For the reaction 2NO2→N2O4+O22\text{NO}_2 \rightarrow \text{N}_2\text{O}_4 + \text{O}_2 , rate expression is as follows: −d[NO2]dt=k[NO2]n, where k=3×10−3 L mol−1 s−1-\frac{d[\text{NO}_2]}{dt} = k[\text{NO}_2]^n, \text{ where } k = 3 \times 10^{-3} \text{ L mol}^{-1} \text{ s}^{-1} If the rate of formation of oxygen is 1.5×10−4 mol L−1 sec−11.5 \times 10^{-4} \text{ mol L}^{-1} \text{ sec}^{-1} , then the molar concentration of NO2\text{NO}_2 in mole L−1\text{L}^{-1} is: (a) 1.5×10−41.5 \times 10^{-4} (b) 0.0151 (c) 0.214 (d) 0.316

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