Question

Review | Constants Periodic Table The following reaction is first order in N, 05: N203(g) + NO3(g) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. Part B You may want to reference (Pages 593 - 598) Section 14.4 while completing this problem. 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. V AXO O2 ? rate = MIS Submit Request Answer 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. IVO AQ R O 2 ? rate = M/S Submit Request Answer
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. You may want to reference (Pages 593 - 598) Section 14.4 while completing this problem. Part A Calculate the rate of the reaction when [N2O5]= 5.7×10−2 M. Express your answer using two significant figures. rate = nothing M/s Request Answer 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 = nothing M/s Request Answer 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 = nothing M/s Request Answer Provide Feedback

Answer 1

Ą [Ngo] 5.7X162 M. k= 0.053 sul Rate = K[Naos] = 0.053 x 5.7x102 = 3.0 x103) M Rate = 0.053x(5.7x162) - 10.2 x10-4 MB Rate - KCNa oslo = [0, 053) Mis