Question

The following reaction is first order in N2O5N2O5: N2O5(g)→NO3(g)+NO2(g)N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s/s.

Part A Calculate the rate of the reaction when [N2O5]=[N2O5]= 5.1×10−2 MM. Express your answer using two significant figures. rate= ______ M/s Part B What would the rate of the reaction be at the same concentration as in Part A if the reaction were second order? (Assume the same numerical value for the rate constant with the appropriate units.) Express your answer using two significant figures. rate = ______ M/s Part C What would the rate of the reaction be at the same concentration as in Part A if the reaction were zero order? Express your answer using two significant figures. rate = _____ M/s

Answer 1

h N205(3)— N03(8) + NO2(6) k= 0.053/5 [N205] = 5.1410-²M * Rate = k [N20s ] = 0.053 5-18 5.1X10-2 mol l-/ = 0:2703 mox 10-2 moll-15-1 Rate - 217X10-3 moli-is-) ③ Rate = k TN 20 s1² second order reaction = 0.0535-' x 5.1X10-2M X 5.1x10-M = 1.37853 X 10=4M25-!| I Rate = 1.4x10-4M25 © Rate = k [N20570 zelo order reaction = 0.0535-1 x 1 Rate = 0.0535-1