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A 1.67-g sample of solid silver reacted in excess chlorine gas to give a 2.21-g sample of pure solid AgCl. The heat given off in this reaction was 1.96 kJ at constant pressure. Given this information, what is the enthalpy of formation of AgCI(s)? O a. -127 kJ/mol O b. 1.96 kJ/mol O C. 127 kJ/mol O d. -63.5 kJ/mol Oe.-1.96 kJ/mol

A 1.67-g sample of solid silver reacted in excess chlorine gas to give a 2.21-g sample of pure solid AgCl. The heat given off in this reaction was 1.96 kJ at constant pressure. Given this information, what is the enthalpy of formation of AgCI(s)? O a. -127 kJ/mol O b. 1.96 kJ/mol O C. 127 kJ/mol O d. -63.5 kJ/mol Oe.-1.96 kJ/mol

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter10: Entropy And The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 10.97PAE
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A 1.67-g sample of solid silver reacted in excess chlorine gas to give a 2.21-g sample of pure solid AgCl. The heat given off in this reaction was 1.96 kJ at constant pressure. Given this information, what is the enthalpy of formation of AgCI(s)? O a. -127 kJ/mol O b. 1.96 kJ/mol Oc. 127 kJ/mol O d. -63.5 kJ/mol O e. -1.96 kJ/mol
Transcribed Image Text:A 1.67-g sample of solid silver reacted in excess chlorine gas to give a 2.21-g sample of pure solid AgCl. The heat given off in this reaction was 1.96 kJ at constant pressure. Given this information, what is the enthalpy of formation of AgCI(s)? O a. -127 kJ/mol O b. 1.96 kJ/mol Oc. 127 kJ/mol O d. -63.5 kJ/mol O e. -1.96 kJ/mol
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