The dissociation vapour pressure (the pressure of gaseous products in equilibrium with the solid reactant) of NH4CI at 427 °C is 608 kPa but at 459 °C it has risen to 1115 kPa. Calculate (a) the equilibrium constant. (b) the standard reaction Gibbs energy, (c) the standard enthalpy, (d) the standardentropy of dissociation, all at 427 °C. Assume that the vapour behaves as a perfect gas and that ΔHΘ and ΔSΘ are independent of temperature in the range given.

The dissociation vapour pressure (the pressure of gaseous products in equilibrium with the solid reactant) of NH4CI at 427 °C is 608 kPa but at 459 °C it has risen to 1115 kPa. Calculate (a) the equilibrium constant. (b) the standard reaction Gibbs energy, (c) the standard enthalpy, (d) the standardentropy of dissociation, all at 427 °C. Assume that the vapour behaves as a perfect gas and that ΔHΘ and ΔSΘ are independent of temperature in the range given.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter10: Effect Of Electrolytes On Chemical Equilibria

Section: Chapter Questions

Problem 10.8QAP

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