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17 Nov 2019
problem 47
was studied at 500. K, and the following data were obtained: Assuming that Rate = Delta[C_4H_6]/Delta t determine the form of the rate law, the integrated rate law, and the value of the rate constant for this reaction. The rate of the reaction O(g) + NO_2(g) rightarrow NO(g) + O_2(g) was studied at a certain temperature. In one experiment, NO_2 was in large excess, at a concentration of 1.0 times 10^13 molecules/cm^3 with the following data collected: What is the order of the reaction with respect to A, and what is the initial concentration of A? Consider the data plotted in Exercise 45 when answering the following questions. What is the concentration of A after 9 s? What are the first three half-lives for this experiment? The reaction A rightarrow B + C is known to be zero order in A and to have a rate constant of 5.0 times 10^-2 mol/L middot s at 25 degree C. An experiment was run at 25 degree C where [A]_0 = 1.0 times 10^-3 M. Write the integrated rate law for this reaction. Calculate the half-life for the reaction. Calculate the concentration of B after 5.0 times 10^-3 s has elapsed assuming [B]_0 = 0. The decomposition of hydrogen iodide on finely divided gold at 150 degree C is zero order with respect to HI. The rate defined below is constant at 1.20 times 10^-4 mol/L middot s. 2HI(g) rightarrow H_2(g) + I_2(g) Rate = Delta [HI]/Delta t = k = 1.20 times 10^-4 mol/L middot s If a initial HI concentration was 0.250 mol/L, calculate the concentration of HI at 25 minutes after the start of the
problem 47
was studied at 500. K, and the following data were obtained: Assuming that Rate = Delta[C_4H_6]/Delta t determine the form of the rate law, the integrated rate law, and the value of the rate constant for this reaction. The rate of the reaction O(g) + NO_2(g) rightarrow NO(g) + O_2(g) was studied at a certain temperature. In one experiment, NO_2 was in large excess, at a concentration of 1.0 times 10^13 molecules/cm^3 with the following data collected: What is the order of the reaction with respect to A, and what is the initial concentration of A? Consider the data plotted in Exercise 45 when answering the following questions. What is the concentration of A after 9 s? What are the first three half-lives for this experiment? The reaction A rightarrow B + C is known to be zero order in A and to have a rate constant of 5.0 times 10^-2 mol/L middot s at 25 degree C. An experiment was run at 25 degree C where [A]_0 = 1.0 times 10^-3 M. Write the integrated rate law for this reaction. Calculate the half-life for the reaction. Calculate the concentration of B after 5.0 times 10^-3 s has elapsed assuming [B]_0 = 0. The decomposition of hydrogen iodide on finely divided gold at 150 degree C is zero order with respect to HI. The rate defined below is constant at 1.20 times 10^-4 mol/L middot s. 2HI(g) rightarrow H_2(g) + I_2(g) Rate = Delta [HI]/Delta t = k = 1.20 times 10^-4 mol/L middot s If a initial HI concentration was 0.250 mol/L, calculate the concentration of HI at 25 minutes after the start of the
Irving HeathcoteLv2
5 Jan 2019