A mixture of 1.00 mol NaHCO3(s) and 1.00 mol Na,CO3(s) is introduced into a 2.50 L flask in which the partial presure of CO2 is 2.10 atm and that of H2O (g) is 715 mmHg. When equilibrium is established at 100°C, will the partial pressures of CO2(g) and H20(g) be greater or less than their initial partial pressures? Explain. 2 NaHCO3(s) = Na2CO3{s) + CO2(g) + H2O(g) Кр = 0.23 at 100 °C

A mixture of 1.00 mol NaHCO3(s) and 1.00 mol Na,CO3(s) is introduced into a 2.50 L flask in which the partial presure of CO2 is 2.10 atm and that of H2O (g) is 715 mmHg. When equilibrium is established at 100°C, will the partial pressures of CO2(g) and H20(g) be greater or less than their initial partial pressures? Explain. 2 NaHCO3(s) = Na2CO3{s) + CO2(g) + H2O(g) Кр = 0.23 at 100 °C

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 36QAP: At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s),...

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