Problem- [Rate Law Problems]The decomposition of N2O5 in carbon tetrachloride proceeds as follows. 2 N2O5 4 NO2 + O2 The rate law is first order in N2O5. At 64°C the rate constant is 4.82 10-3 s-1.
1) Write the rate law for the reaction. rate = k[4NO2][O2] / [N2O5] rate = k[N2O5] rate = k[4NO2]2[O2] / [N2O5] (this part i figured out.)
2) What is the rate of reaction when [N2O5] = 0.0235 M? M/s
3) What would the rate be when the concentration of N2O5 is doubled to 0.0470 M? M/s
Explain the each and every step in detail for help