14.54 Heating solid sodium bicarbonate in a closed vessel establishes the following equilibrium: 2NAHCO3(s) = Na,CO3(s) + H2O(g) + CO2(g) What would happen to the equilibrium position if (a) some of the CO2 were removed from the system; (b) some solid Na,CO3 were added to the system; (c) some of the solid NaHCO3 were removed from the system? The temperature remains constant.

14.54 Heating solid sodium bicarbonate in a closed vessel establishes the following equilibrium: 2NAHCO3(s) = Na,CO3(s) + H2O(g) + CO2(g) What would happen to the equilibrium position if (a) some of the CO2 were removed from the system; (b) some solid Na,CO3 were added to the system; (c) some of the solid NaHCO3 were removed from the system? The temperature remains constant.

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

51.0 g of Y(g) (molar mass = 28.32 g/mol) is placed in a 0.617 L flask for the following reaction to take place. Calculate the concentration (molarity) of Z equilibrium. The equilibrium constant for the reaction is K = 4.63 x 10-4 at 25°C. Report your answer to the thousandths place. Y(g) = 2 Z(g)
A student ran the following reaction in the laboratory at 675 K: H2(g) + I2(g) 2HI(g) When she introduced 0.226 moles of H2(g) and 0.248 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.11×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
A student ran the following reaction in the laboratory at 1097 K: 2SO3(g)2SO2(g) + O2(g) When she introduced 0.0921 moles of SO3 (g) into a 1.00 liter container, she found the equilibrium concentration of O₂ (g) to be 0.0198 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
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 student ran the following reaction in the laboratory at 431 K: PCI 5(9) PC13(g) + Cl₂(9) When she introduced 2.02 moles of PCI5(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.08x10-² M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
Compare the following two reactions ("A" and "B"), with two different equilibrium constants, K: (A) Cl2 (g) + H2 (g) = 2HCI (g) K = 0.29 (B) I2 (g) + H2 (g) = 2HI (g) K = 1.6 x 1033 %3D Which of the following statements is correct? O Reaction "A" will proceed faster because the equilibrium constant, K, is larger O Reaction "B" will proceed faster because the equilibrium constant, K, is larger O Reaction "A" favors the production of products. O Reaction "B" favors the production of products. O None of these statements are correct.
Calculating an equilibrium constant from a partial equilibrium composition Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 2.0 L flask with 1.2 atm of ammonia gas and 3.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.3 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = [] P x10 X ? olo 18 Ar 8.