Consider this reaction: CH3H|| + HCl = CH3HgCl + HI Which is the correct prediction and explanation about the equilibrium constant, K, for this reaction? OK> 1, because I is a harder base than Cl. K< 1, because l is a harder base than Cl.. K > 1, because Cl is a harder base than I. OK< 1, because Cl is a harder base than I.

Consider this reaction: CH3H|| + HCl = CH3HgCl + HI Which is the correct prediction and explanation about the equilibrium constant, K, for this reaction? OK> 1, because I is a harder base than Cl. K< 1, because l is a harder base than Cl.. K > 1, because Cl is a harder base than I. OK< 1, because Cl is a harder base than I.

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...

See similar textbooks

Similar questions

Given a solution of acetic acid, with equilibrium net ionic equation (so only showing the ions in the reaction and not the spectator ions): CH3COOH (aq) + H20 () CH3COO (aq) + H3O* (aq) Have 4 beakers with acetic acid. Each beaker gets one of the following four things added to it. Match each thing with how the equilibrium responds when the thing is added. Prompts Submitted Answers sodium acetate Choose a match calcium acetate nothing sodium chloride shifts left to make more reactants acetic acid shifts right then left then right then left... shifts right to make more products
2H2O ⇆ H3O+ + OH- To decrease the concentration of OH- ions in the equilibrium above, you could a. add an acid to the solution b. add a base to the solution c. add a catalyst to the solution d. more than one choice is correct
When the equation 2SO2 (g) + O2 (g) E 2 SO3 (g) came to equilibrium, the concentration of reactants and products were as follows: [SO3] = 0.40M; [SO2] = 0.15 M ; [02] = 0.20 M. Calculate the equilibrium constant (Keg) for this reaction. Oa. 13 м1 Ob. b. 0.72 M-1 С. 0.028 M-1 Od. 36 M-1
What is the equilibrium constant, Kc, of the following reaction when [PCl5] = .200 M, [PCl3] = .040 M, [Cl2] = 0.080 M pci5(g)⇌ pci3(g)+ci2(g) A. 62.5 C. 0.016 D. 1.54
H2 + Cl2 à HCl for which the equilibrium constant K = 320 at 150 C. Suppose 0.400 mol of H2 and 0.300 mol of Cl2 were placed in a 1.5-liter vessel at 250 C. What will the concentrations of all species be once equilibrium is established?
1. Consider the reaction below. Co(H,0), (aq) + 4 CF (aq) = CoCl (aq) + 6 H20 (1) The equilibrium constant expression (K) of the reaction does not include the concentration of H,0 even though the reaction produces six moles of water. Explain.
Quickly please
For the next items, refer to the following information on a hypothetical acid, HA. Consider a hypothetical acid, HA, solution with a concentration of 0.1 M. The Ka value of HA at 25°C is 1 x 10-3. [НA], M [H*), M [A-], M Initially Change Equilibrium
at 200 ° C, the numerical value of Kc for the following reaction is 8 × 10-³. PCl5 = PCl3 + Cl2 deltaH = + 124 kj / mol a) How would it affect the value of the equilibrium constant if: i.add PCl5 ii.pressure increases iii.the temperature rises.
2H2O ⇆ H3O+ + OH- To decrease the concentration of OH- ions in the equilibrium above, you could a. add an acid to the solution b. add a base to the solution c. add a catalyst to the solution d. more than one choice is correct
For the reaction below, Kc = 1.10 × 10-8. Note Kc is sometimes called K. What is the equilibrium concentration of OH- if the reaction begins with 0.270 M HONH2? HONH2 (aq) + H2O () = HONH3+ (aq) + OH- (aq)
Write the basic equilibrium equation for C,H,NH, 3. O4- D2. O+ n2+ O3+ O4+ 1 2 3 4 7 8 1 3 4 5 O6 (s) (1) (g) (aq) + -> H C OH Reset • a H,O Delete 80 888 F3 F4 F5 F6 F7 FB 2# $ % & * 3 4 5 6 7 9 W E R Y U CO