Heating BaCO3 leads to decomposition: BaCO3 (s) → BaO (s) + CO2 (g) AH = 15.7 kJ/mol a) If the reaction flask is heated, how does the pressure of the CO2 change? b) If the mass of BaCO3 is increased from 5.0 g to 10.0 g, how does the pressure of CO2 change? c) If the volume of the container is doubled, which direction does the equilibrium reaction shift (if any) to re-establish a state of equilibrium?

Heating BaCO3 leads to decomposition: BaCO3 (s) → BaO (s) + CO2 (g) AH = 15.7 kJ/mol a) If the reaction flask is heated, how does the pressure of the CO2 change? b) If the mass of BaCO3 is increased from 5.0 g to 10.0 g, how does the pressure of CO2 change? c) If the volume of the container is doubled, which direction does the equilibrium reaction shift (if any) to re-establish a state of equilibrium?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.108QE

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