The following reaction is first order in N2O5: N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s.?
What would the rate of the reaction be at the same concentration as in part a if the reaction were second order? or Zero order?(Assume the same numerical value for the rate constant with the appropriate units.)
Express your answer using two significant figures.
- hcbiochemLv 71 month ago
For a second order reaction, the rate law would be:
rate = k [N2O5]^2
rate = 0.053 [N2O5]^2 = _______
You didn't provide a concentration of N2O5 to use in this calculation.
For a zero order reaction, the rate law is simply rate = k = 0.053 M/s