The gas-phase reaction between hydrogen and iodine
s and an activation energy of 165 kJ/moI.
(a) Calculate the activation energy of the reverse reaction given that
(b) Calculate the rate constant for the reverse reaction at 700°C. (Assume A in the equation
(c) Calculate the rate of the reverse reaction if the concentration of HI is 0.200 M. The reverse reaction is second-order in HI.
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Chapter 11 Solutions
Chemistry: Principles and Reactions
- The element Co exists in two oxidation states, Co(II) and Co(III), and the ions form many complexes. The rate at which one of the complexes of Co(III) was reduced by Fe(II) in water was measured. Determine the activation energy of the reaction from the following data: T(K) k (s-1) 293 0.054 298 0.100arrow_forward2a) Briefly explain, in your own words, the difference between the "activation energy" of a reaction and the "net free energy change" of a reaction.arrow_forwardThe rate law for the reaction rate is: k[A]^2[B]arrow_forward
- What is the activation energy for a reaction if k= 1.89 X 10^-8 s^-1 at 540 degrees Kelvin and k= 2.45 X 10^-7 s^-1 at 601 degrees Kelvin?arrow_forwardConsider the reaction : 3A + 2B → 4C Initially, and at some fixed temperature, the reaction proceeds at such a rate that 2.3 millimoles of A are consumed in 1 minute and 12 secondes. The reaction takes place in 1 L. The following table contains the experimental data for the reaction. (Taken from Ball. Physical Chemistry, 2nd edition, 2006) Rate (M/s) [A], M [B], M 1.081 x 10-5 0.660 1.23 6.577 x 10-5 4.01 1.23 6.568 x 10-5 4.01 2.25 d. What is the order of the reaction. e. Express the rate law and the integrated form equation. Is the reaction elementary? f. If the rate constant k = 1.61x10-5s-1 and [A0] = 4M, find the period of time between the 12th and 13th half-life. *g. If, for the same reaction, at the same temperature, we were to add a catalyst, would Ea, A, k and v be larger, smaller or equal? Explain.arrow_forwardConsider the reaction : 3A + 2B → 4C Initially, and at some fixed temperature, the reaction proceeds at such a rate that 2.3 millimoles of A are consumed in 1 minute and 12 secondes. The reaction takes place in 1 L. The following table contains the experimental data for the reaction. (Taken from Ball. Physical Chemistry, 2nd edition, 2006) Rate (M/s) [A], M [B], M 1.081 x 10-5 0.660 1.23 6.577 x 10-5 4.01 1.23 6.568 x 10-5 4.01 2.25 c. Determine the partial order on A. Partial order on B is 0. d. What is the order of the reaction.arrow_forward
- The activation energy for the reaction A2(g) ! B2(g) 88n 2AB(g) is 167 kJ/mol, and $E for the reaction is !28 kJ/mol. What is the activation energy for the decomposition of AB?arrow_forwardIn the following chemical reaction A + B → 2C + 40KJ at a certain temperature, if you know that the potential energy of the reactants is 80 kilojoules, and the potential energy of the activated complex is 160 kilojoules, and when a catalyst is added, the activation energy for the forward reaction becomes 50 kilojoules, a. What is the value of the activation energy for a reverse reaction in kilojoules in the presence of the catalyst? And without the catalyst? b. What is the value of the potential energy (in kilojoules) of the products of a chemical reaction? c. What is the value of the activated Complex potential energy (in kilojoules) in the presence of the catalyst?arrow_forwardEnzymes in the human liver catalyze a large number of reactions that degrade ingested toxic chemicals. By what fac-tor is the rate of a detoxification reaction changed if a liver enzyme lowers the activation energy by 5 kJ/mol at 37°C?arrow_forward
- For the following reaction producing 1 mol of oxygen gas at a particular temperature, ΔH = –180 kJ. NO(g) + O3(g) → NO2(g) + O2(g) The activation energy is 11 kJ/mol. What is the activation energy for the reverse reaction?arrow_forwardA particular second-order reaction has a rate constant of 2.4 x 10–6 M–1 s–1 at 575 K and 6.0 x 10–5 M–1 s–1 at 630 K. (a) Calculate the activation energy of the reaction. (b) What is the value of the rate constant at 25°C?arrow_forwardwhat is the effect on k as the activation energy for a reaction increasesarrow_forward
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