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Given the reaction 2NH4NO3(s)+Ba(OH)2(s) => 2H2O1) + 2NH3(g) + Ba(NO3)2(s), AH°RX = +196 kJ, and relevant AH°F values, calculate the heat of formation of NH4NO3(s). Show work. Don't look at the thermodynamic values table. AH°f values: Ba(OH)2(s) = - 946KJ/mol, H2O) = - 286 Ba(NO3)26) = -990 kJ/mol, NH3) = -46 kJ/mol, kJ/mol

Given the reaction 2NH4NO3(s)+Ba(OH)2(s) => 2H2O1) + 2NH3(g) + Ba(NO3)2(s), AH°RX = +196 kJ, and relevant AH°F values, calculate the heat of formation of NH4NO3(s). Show work. Don't look at the thermodynamic values table. AH°f values: Ba(OH)2(s) = - 946KJ/mol, H2O) = - 286 Ba(NO3)26) = -990 kJ/mol, NH3) = -46 kJ/mol, kJ/mol

Chemistry
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...
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Is the answer 452 kJ or - 402 kJ
Given the reaction 2NH4NO3(6)+Ba(OH)2(s) => 2H2O(1) + 2NH3(g) + Ba(NO3)2(s), AH°RX = +196 kJ, and relevant AH°F values, calculate the heat of formation of NH4NO3(s). Show work. Don't look at the thermodynamic values table. AH°f values: Ba(OH)2(s) = - 946KJ/mol, H2O) = - 286 kJ/mol, NH3) = -46 kJ/mol, Ba(NO3)26) = -990 kJ/mol
Transcribed Image Text:Given the reaction 2NH4NO3(6)+Ba(OH)2(s) => 2H2O(1) + 2NH3(g) + Ba(NO3)2(s), AH°RX = +196 kJ, and relevant AH°F values, calculate the heat of formation of NH4NO3(s). Show work. Don't look at the thermodynamic values table. AH°f values: Ba(OH)2(s) = - 946KJ/mol, H2O) = - 286 kJ/mol, NH3) = -46 kJ/mol, Ba(NO3)26) = -990 kJ/mol
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