Part AFor a certain reaction, K. = 25.5 and kg = 33.3 M2.s1. Calculate the value of the reverse rate constant, k,, given that the reverse reaction is of the samemolecularity as the forward reaction.Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M.s include (multiplication dot)between each measurement.> View Available Hint(s)k =ValueM2 s 1SubmitPart BFor a different reaction, K. 103, kg = 6.76 × 10°s, and k, = 65.7 s-1. Adding a catalyst increases the forward rate constant to 9.73x105 s-1 What is the newvalue of the reverse reaction constant, k, after adding catalyst? 37 of 37Item 37Part BFor a different reaction, K. 103, k = 6.76 x 10°s=1, and k, = 65.7 s-1 Adding a catalyst increases the forward rate constant to 9.73x105 s1 What is the newvalue of the reverse reaction constant, k, after adding catalyst?Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M.s-1 include (multiplication dot)between each measurement.> View Available Hint(s)k, =Values 1SubmitPart CYet another reaction has an equilibrium constant K. = 4.32 x 10° at 25 °C. It is an exothermic reaction, giving off quite atemperature is raised to 200 °C, what will happen to the equilibrium constant?of heat while the reaction proceeds. If the

Kc = 25.5 Kf = 33.3 M-2 s-1 Kb = ?

For a certain reaction, K. = 25.5 and k = 33.3 M.s. Calculate the value of the reverse rate constant, k, given that the reverse reaction is of the same molecularity as the forward reaction. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M.s include (multiplication dot)

For a certain reaction, K. = 25.5 and k = 33.3 M.s. Calculate the value of the reverse rate constant, k, given that the reverse reaction is of the same molecularity as the forward reaction. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M.s include (multiplication dot)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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HW 18 Solve question 11 Use answer box below
For the following reaction, the Kc is 1.89 at 933K. H2(g) + CO2(g) H20(g) + CO(g) Calculate the equilibrium concentration of hydrogen, [H2], when [CO2] = 0.210M, [H2O] = 0.390M, and [CO] = 0.160M. A. 0.124M В. О.103М С. 2.84М D. 0.074M
the numbers 1-3 are just sub questions, thank u!!
Be sure to answer all parts. The equilibrium constant Ke for the reaction H₂(g) + CO₂(g) = H₂O(g) + CO(g) is 4.2 at 1650°C. Initially 0.75 mol H₂ and 0.75 mol CO₂ are injected into a 4.8-L flask. Calculate the concentration of each species at equilibrium. Equilibrium concentration of H₂: M Equilibrium concentration of CO₂: M Equilibrium concentration of H₂O: M Prex 17 of 27 ‒‒‒ -
Consider the reaction CH₂O(g) = H₂(g) + CO(g). Exactly 3.4E-2 moles of CH₂O were injected into a 250 mL flask. At equilibrium, [CH₂O]=6.2E-2 M. What is Ke for this reaction? ir notation (Uso Enotation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 10°)
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For the reaction below, Kc = 0.60 at 550 K. The reaction starts with a 0.050 M concentration of A2B2, at 550 K. A₂B₂ (g) = 2 AB (g) In crafting a RICE table as modeled in class, what is the expression for the product from equilibrium row of RICE table? You can disregard sign (whether it is positive or negative). O X 2x ~ 2x²
Consider the following reaction CO(g) + 2H₂(g) CH₂OH(g) The reaction between CO and H₂ is carried out at a specific temperature with initial concentrations of CO 0.29 M and H₂ 054 M At equilibrium, the concentration of CH₂OH is 0.16 M Part A Find the equilibrium constant at this temperature. Express your answer using two significant figures. 195] ΑΣΦ Submit Previous Answers Request Answer ?
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Part A The reaction below is carried out at a different temperature at which Ke = 0.055. This time, however, the reaction mixture starts with only the product, NO = 0.0100 M, and no reactants. Find the equilibrium concentrations of N2, O2, and NO at equilibrium. N2(8) + O2(g) = 2NO(g) Express your answers to three significant figures separated by commas. > View Available Hint(s) ? [N2]. [O2]. [NO] = М, М, М Submit Provide Feedback Next >
Calculate the Keg from the given concentrations, all are gases. C2H6 1.000 M 2 Cl2 1.000 M C2H4CI2 + 0.000 M 0.250 M + 2 HCI start: 0.000 M equilibrium: 0.750 M 0.500 M 0.500 M 0.500 M used First put in the chemicals, then put in the numbers. The concentrations for both Cl2 and HCl are squared due to their coefficients. [ Kea %3D Keg = a. H3O*1 b. Он1 c. C2H6 d. C2HĄCI2 e. Cl2 f. HCI g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS-1 I. s2 m. HX п. X1 o. 0.750 р. 2 q. 1 r. 0.250 s. 0.500 t. 0.333 u. 8.00 х 10-5 v. 1.75 x 10-6 w. 1.11 x 10-8 x. 5.5 x 10-2 у. О.7000 z. 1.60 x 10-5 aа. 1.143 х 10-5 bb. 0.6000 СС. 1.104 х 10-5 dd. 0.7100 ее. 1.26 х 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957
The ff. equilibrium constants have been determined for Phosphoric acid (H3PO4) at 25oC. K’c = 3.5 x 10 -4 K’’c = 4.6 x 10-5 K’’’c = 4.8 x 10-6 What is the equilibrium constant (Kc) for the overall reaction? Note: Express your final answer in scientific notation. Round off into 2 decimal places. Example: 1.11 x 10-11 or 1.11 x 10^(-11)