Consider the reaction: 2 CO(g) + O₂(g)=2 CO₂(g). ↑ The reaction is allowed to reach equilibrium in a sealed vessel. According to Le Chatelier's principle, what will happen to the equilibrium, if the volume of the vessel is decreased while the temperature is kept constant? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will be unchanged, but the reaction will shift to the right. (D) The equilibrium constant will increase and the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.

Consider the reaction: 2 CO(g) + O₂(g)=2 CO₂(g). ↑ The reaction is allowed to reach equilibrium in a sealed vessel. According to Le Chatelier's principle, what will happen to the equilibrium, if the volume of the vessel is decreased while the temperature is kept constant? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will be unchanged, but the reaction will shift to the right. (D) The equilibrium constant will increase and the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.

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

Sulfuric acid is produced through the contact process, which involves the catalytic oxidation of sulfur dioxide as an intermediate reaction: 2SO2(g) + O2(g) ⇋ 2SO3(g). Write the equilibrium expression for this process.
A student ran the following reaction in the laboratory at 600 K: CO(g) + Cl₂(g) —COCI₂(g) When he introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 2.09 atm and the initial partial pressure of Cl₂ was 1.22 atm, he found that the equilibrium partial pressure of Cl₂ was 0.405 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр
Consider the following equilibrium: NH3(g) + HCl(g) NH4CI(s) Suppose a vessel containing NH4Cl(s), NH3(g) and HCl(g) is at equilibrium. If the volume of the vessel is instantaneously doubled while keeping the temperature constant, when a new equilibrium is reached, which of the following statements is incorrect? The partial pressures of NH3 and HCI in the vessel remain unchanged. The total pressure is halved. O The value of Kp remains unchanged. O The number of moles of NH4Cl decreases. O The amount of NH3 and HCI doubles.
The reaction is at equilibrium at some temperature, T, and the following equilibrium concentrations are measured: [SO2] = 0.90 M, [O2] = 0.35 M, and [SO3] = 1.1 M. Write the equilibrium expression for this reaction. Calculate Keq for the reaction at temperature, T.
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 5.96 × 104: H₂(g) + Cl₂(g) →2 HCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 1.8 mol of HCI. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 HCl(g) H₂(g) + Cl₂(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 H₂(g)+2Cl₂(g) 4 HCl(g) ܢܢ There will be very little H₂ and Cl₂. There will be very little HCI. Neither of the above is true. K = 0 K = 0 x10 X 0/3 ? olo 18 Ar BA
Define equilibrium constant Keq
8) Consider the system below. When equilibrium is restored, how will the number of each type of molecule and the concentration of each substance compare to those before the stress was introduced? Complete the following table using the words "decrease," "same," or "increase." 2 NH,(g) = N,(g) + 3 H,(g) AH = 92.4 kJ/mol Decrease Volume Decrease Temperature N, Equilibrium Concentration Н, NH, N, Equilibrium Number Н, NH,
Suppose the following reaction is at equilibrium: PCl3 + Cl2 ⇋ PCl5. (a) Are the equilibrium concentrations of PCl3, Cl2, and PCl5 necessarily equal? Explain. (b) Is the equilibrium concentration of PCl3 necessarily equal to that of Cl2? Explain.
Consider the following exothermic reaction at equilibrium: N2 (g) + 2H2 (g) ⇌ 2NH3 (g) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below. Complete the table with the terms increase, decrease, or no change
Consider the following equilibrium for which H = 180.74: N2(g) + O2(g) 2 NO(g) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction?(a) NO(g) is added to the system. (b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%. (d) A catalyst is added to the reaction mixture. (e) The total pressure of the system is increased by adding a noble gas. (f) O2(g) is removed from the system.
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 N, (g) + 3 H, (g) = 2 NH3 (g) К, — 3. х 10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 3.2 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes x10 tools available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of NH, at right. atm Round your answer to 1 significant digit.