Rank the following reactions from most reactant-favored to least reactant-favored. B: K = 9.1x10-4 C: K= 2.7x10-3 D: K=1.7x10-5 3) A: K= 1.7x10-³ most reactant-favored: least reactant-favored 4) A mixture of carbon monoxide, hydrogen, and methanol is at equilibrium at 25°C. The balanced chemical equation is: CO(g) + 2H₂(g) = CH₂OH(g). At equilibrium, the mixture contains 0.0960 M CO, 0.191 M H₂, and 0.204 M CH3OH. What is the value of Ke at this temperature?

Rank the following reactions from most reactant-favored to least reactant-favored. B: K = 9.1x10-4 C: K= 2.7x10-3 D: K=1.7x10-5 3) A: K= 1.7x10-³ most reactant-favored: least reactant-favored 4) A mixture of carbon monoxide, hydrogen, and methanol is at equilibrium at 25°C. The balanced chemical equation is: CO(g) + 2H₂(g) = CH₂OH(g). At equilibrium, the mixture contains 0.0960 M CO, 0.191 M H₂, and 0.204 M CH3OH. What is the value of Ke at this temperature?

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

What is the chemical equilibrium expression for the equation 2A,B + 3CD AD + C3B2? O [4,B]°[CD] [A,D][C,B,] O 6[A,B][CD] TA,D][C,B,] O [A,D][C,B,] [A,B]°[CD] O [A,D][C,B,] 6[A,B][CD]
2. Ozone can be created from oxygen gas (with an input of energy) via the following reaction: 30₂(8) = 203 (8) -2 If the equilibrium constant, K, is 1.02 x 10-24 for this reaction at a particular temperature and [0₂] = 3.10 x 10 M at equilibrium, what is [03] (in M to two decimal places) at equilibrium? A: 5.51 x 10 -15 (2) (028 DES (2)₂0+ (₂),025 = (8)¿025
kJ/mol +410 kJ/mol LLEGES 20 O-410 kJ/mol Question 12 Give the equilibrium constant expression for the reaction 2HBr2(g) Br₂(g) + H₂(g) OK= [Br2] [H₂] / [HBr] OK= [Br₂] [H₂]/[HBr] OK [HBr]2/[Brz][H₂] OK-2[HBr]2/(2[Br₂] x 2[H₂1) OK [Br2] [H₂]²/[HBr] 121666 3
4. The reaction X + Y 2 Z is one that essentially goes to completion at equilibrium. Which of the following values is most likely the Kc for this reaction? a) 2.6 x 10-18 b) 3.5 x 10-2 c) 1.00 d) 4.7 x 105 e) 1.06 x 10-14
One of the steps in the production of sulfuric acid involves the catalytic oxidation of sulfur dioxide. 2 SO2 (g) + O2 (g) → 2 SO3 (g) What is the equilibrium expression?
None
The standard Gibbs free energy, ∆??, is:a) The residual energy present in the reactants in the equilibrium stateb) The residual energy present in the products in the equilibrium statec) The difference in the residual energy of the reactants and products inBalance.d) The energy required to convert one mole of reactants into one mole ofproducts[justify the answer you consider correct]
С. 4 NH3(g) + 5 O2(g) 5 4 NO(g) + 6 H20(g) + heat Stress applied: Increasing the volume of the container 1. What is the Keq expression? 2. What will be the effect in the amount of H2O? 3. What will be the Equilibrium Shift or the reaction?
The following reaction is product-favored at equilibrium at room temperature. C,H2 (g) + H2 (g) → C,H4 (g) Will raising or lowering the temperature make it reactant-favored? Raising the temperature can make it reactant-favored. O Lowering the temperature can make it reactant-favored. O Neither raising nor lowering the temperature can make it reactant-favored.
Consider the reaction: SO₂(g) + 1/2O₂(g) ⇒ SO3 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: 2S(s) + 30₂(g) ⇒ 2SO3 (9) K₁ S(s) + O₂(g) → SO₂(g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K= An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.
Which of the following statements is TRUE? If Q < K, the reaction proceeding to the left is much faster than the reaction proceeding to the right. If Q < K, it means the reverse reaction will proceed to form more reactants. Because the equilibrium is always dynamic, Q can never be equal to K. If Q = K, it means the reaction is not at equilibrium. If Q > K, it means the reverse reaction will proceed to form more reactants.
Which reaction has the smallest equilibrium constant?