Question 17Express the equilibrium constant for the following reaction.2 CH3CI(g) + Cl2(g) → 2 CH2C12(g) + H2(g)is supposed to be an equilibrium arrow.[CH2C12][H2][CH3CI][Cl2]K =[CH;Cl2}[H2][CH;CI]°[Cl2]K =[CH;CI}{[Cl2][CH,Cl2f[H2]K =[CH;CI][Cl2][CH2C12][H2]K =[CH;CI] 7 [Clz]K =[CH¿Cl2]7 [H2]

Answered: Image /qna-images/answer/02f91515-c222-4f0b-8afd-14c2f5b7c4b0.jpg

Question 17 Express the equilibrium constant for the following reaction. 2 CH3CI(g) + Cl2(g) → 2 CH2CI2(g) + H2(g) is supposed to be an equilibrium arrow. [CH2C12][H2] [CH3CI][Cl2] K = [CH2Cl½f[H2] [CH;CI]°[Cl2] K = [CH;CI}*[Cl>] [CH,Cl2f[H2] K = [CH;CI][Cl2] [CH2C12][H2] K = [CH;CI] 7 [Clz] K = [CH;Cl2]² [H2]

Question 17 Express the equilibrium constant for the following reaction. 2 CH3CI(g) + Cl2(g) → 2 CH2CI2(g) + H2(g) is supposed to be an equilibrium arrow. [CH2C12][H2] [CH3CI][Cl2] K = [CH2Cl½f[H2] [CH;CI]°[Cl2] K = [CH;CI}*[Cl>] [CH,Cl2f[H2] K = [CH;CI][Cl2] [CH2C12][H2] K = [CH;CI] 7 [Clz] K = [CH;Cl2]² [H2]

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

Can you show me how to answer this type of question I found on a online practice organic chemistry review.
Hydrogen lodide is produced by combining hydrogen gas and iodine gas as shown in the balanced chemical reaction below. If H2 and 12 each have an Initial pressure of 1.73 atm, what is the equilibrium pressure of HI? The equilibrium constant for the reaction is 137. H2 (9) + 12 (9) = 2HI (g) Report your answer to two decimal places. Do not put a unit. A Moving to another question will save this response. Question 12 of 30
In a flask containing the reaction, PCI3(g) + Cl2(g) = PCI5(g), equilibrium concentrations were found to be 1.88 M PCI3 and 1.86 M Cl2. What is the equilibrium concentration of PCIl5 (M) if the equilibrium constant is 4.6 x 104?
Examine the following equilibrium: MgO (s) + CO₂ (g) = MgCO3 (s) The correct formula for the equilibrium expression is: OKeq = Keq [MgCO3] Keq = MgO][CO₂] = 1 [CO] [MgCO3] [CO₂] Keq = [CO₂]
Consider the following reaction: 2 H20(g) + 2 SO2(g) = 2 H2S(g) + 3 O2(g) A reaction mixture initially contains 2.8 M H20 and 2.6 M SO2. If the equilibrium concentration of H2S is 0.112 M, find the equilibrium constant (Kc) for the reaction.
My question is below. Any help would be appreciated. Consider the following reaction: CO (g) + 2 H2 (g) = CH3OH (g) A reaction mixture in a 5.15 L flask at a certain temperature initially contains 27.1 g CO and 2.32 g H2. At equilibrium, the flask contains 8.65 g CH3OH. Calculate the equilibrium constant (Kc) for the reaction at this temperature.
Consider the following reactions: CO(g) + H20(g) +→CO2(g) + H2(g) K = 1.33 x 105 COlg) + 2 H2(g) +CH3OH(g) K2 = 2.59 x 107 Determine the value of the equilibrium constant for the following reaction: CO2(3) + 3 H2(g) → CH3OH(g) + H2O(g)
Consider the reaction, PCI5(g) = PCI3(g)+ Cl2(g) where the value for Kc is 5.1 x 10- 5. The initial concentration of PCI5 is 1.16 M. What is the concentration (molarity) of PCI3 at equilibrium? Report your answer to two decimal places using scientific notation. X ÷ T ab ab () ?
What is the value for this equation? Given: CO(g)+H20(g)=CO2(g)+H2(g) = 1.0 and initial concentrations are [CO2(g)]= 2.0 M, [H2(g)]= 2.0 M, [CO(g)]= 1.0 M, [H2O(g)]= 1.0 M
For the steam hydrocarbon reforming process, the equilibrium law expression is [CO₂(g)][H₂(g)]* [CH][H₂0² Kc The reaction described by this equilibrium is CH4 (a) + H₂O(g) = CO₂(g) + H₂(g) CH4 (q) + 2H₂O(g) = CO₂(g) + 4H₂(g) CO₂(g) + 4H₂(g) = CH₁ (a) +2H₂O(g) CO₂(g) + H₂ (a) CH4 (q) + H₂O(g)
Suppose a 250. mL flask is filled with 0.20 mol of N2 and 2.0 mol of NO. The following reaction becomes possible: N2(g) + O2(g) = 2NO(g) The equilibrium constant K for this reaction is 0.693 at the temperature of the flask. Calculate the equilibrium molarity of N2. Round your answer to two decimal places. Шм
Consider the following equilibria: 2SO3(g) 2SO2(g) + O2(g) Kc1 = 2.3 × 10 – 7 2NO3(g) ⟷ 2NO2(g) + O2(g) Kc2 = 1.4 ×10 – 3 Calculate the equilibrium constant for the reaction: SO2(g) + NO3(g) ⟷ SO3(g) + NO2(g) A 1.3 × 10 – 2 B 1.6 × 10 – 4 C 78 D 6.1 × 103