Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- 6) The decomposition of reactant R was studied, and the data given below was obtained at 100.0 °C: R> products time (min) concentration (M) 0.120 35.6 5.83 17.8 25.6 0.0910 0.060 0.046 0.030 a) What is the half-life of the reaction in minutes? Explain. b) Various plots of the concentration of the reactant versus time are given below. What is the order of the reaction? Explain. ILD is 20 time (min) time (min) 05 -35 time (min) c) What is the value of the rate constant at 100.0 °C? d) Would you expect the half-life of the reaction to be longer, shorter, or the same at 60.0 °C? Explain. e) The activation energy in the forward direction is 95.0 kl/mol, and the enthalpy change for the forward reaction is 30.0 kl/mol. Sketch the reaction coordinate diagram for this reaction. ERER ARarrow_forward(c) A reaction between substances R and S was second order with respect to R and second order with respect to S. S-or x 8.1 0.3 At a given temperature, the initial rate of reaction was 1.20 x 10-3 mol dm-3 s-1 when the initial concentration of R was 1.00 x 10-2 mol dm-3 and the initial concentration of S was 2.45 x 10-2 mol dm-3 acom ton Scor 0.8 Calculate a value for the rate constant, k, for the reaction at this temperature. Give the units for k rose ni to nollbeen to stist leitini ert worla of SeldsT otalama) (B) S eldsT amb tom \\ els fallinl Ot *8.1 Inomheqx3arrow_forwardA certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [1] initial rate of reaction 1.50 M 2.34 M 77.0 M/s O M/s 2.12 M 2.34 M O M/s 0.300 M 11.7 Marrow_forward
- Be sure to answer all parts. Rep Consider the reaction A+B Products From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. [A] (M) [B] (M) Rate (M/s) 1.50 1.50 3.20 x 10 1.50 2.50 3.20 x 10 Reaction 3.00 1.50 6.40 x 10 Proctorio is shaning your screen. Stop sharingarrow_forwardA certain reaction is first order in H, and first order in I,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [H.] [1] initial rate of reaction 1.10 M 0.547 M 16.0 M/s I M/s 2.43 M 0.547 M I M/s 2.20 M 0.273 Marrow_forwardA certain reaction is second order in N, and second order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N-] initial rate of reaction 0.153 M 1.80 M 13.0 M/s x 5 ? 0.245 M 1.80 M O MIs 0.618 M 0.445 M M/sarrow_forward
- A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [H.] initial rate of reaction 1.89 M 2.21 M 6.00 x 10° M/s I M/s 1.89 M 0.910 M 2.37 M 1.76 Marrow_forwardA certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [H,] initial rate of reaction x10 2.37 M 0.112 M 0.123 M/s alo ) 2.37 M 0.0539 M M/s 18 Ar 0.339 M 0.784 M | M/sarrow_forward3) Rate (M/s) 0.7 0.6 0.5 0.4 0.3 0.2 0.1 0 Reaction Data 0.1 0.2 0.3 0.4 0.5 [A] (M) Use the experimental data to answer. a) What is the order of reaction with respect to A? b) What is the rate coefficient k? c) Write the rate law. 0.6 0.7 0.8 0.9 1arrow_forward
- A certain reaction is second order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [4] Initial rate of reaction 2.41 M 0.733 M 19.0 M/s 0.501 M 0.733 M Mls 0.873 M 2.02 M Mls dlo Ararrow_forwardThe decomposition of a chemical follows the Zero order with a rate constant, k = 0.00543 M/s. If the initial concentration of the reactant is 2.32. what is the concentration after 900 seconds?. The decomposition of a chemical is in the second order with a rate constant, k = .0123 M-1min-1. If the initial concentration of the reactant is 0.765 M. What is the concentration after 15 minutes.arrow_forwardThe following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NO + 03 NO₂ + O₂ Experiment [NO]o, M [03]o, M Initial Rate, M-s1 0.192 0.0497 0.928 0.192 0.0994 1.86 0.384 0.0497 1.86 0.384 0.0994 3.71 1 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or 71. Rate = k= Marrow_forward
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