1. Determine the amount of energy released when 93.6 g of liquid butane, C,H10(1 combusted. AH,°(CO2(g)) = -393.5 kJ/mol; A H; °((H20(1)) = -285.8 kJ/mol; AH÷°((C,H10(1)) = -147.6 kJ/mol) Write the formation reactions for the following substances:
1. Determine the amount of energy released when 93.6 g of liquid butane, C,H10(1 combusted. AH,°(CO2(g)) = -393.5 kJ/mol; A H; °((H20(1)) = -285.8 kJ/mol; AH÷°((C,H10(1)) = -147.6 kJ/mol) Write the formation reactions for the following substances:
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 5.62QE: A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup...
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Transcribed Image Text:1. Determine the amount of energy released when 93.6 g of liquid butane, C,H,0(1), is
combusted. AH,°(CO2(g)) = -393.5 kJ/mol; A H; °((H,0(1)) = -285.8 kJ/mol;
%3D
AH,°((C,H10(1)) = -147.6 kJ/mol)
2. Write the formation reactions for the following substances:
solid aluminum chloride, AH,°= -704.9 kJ/mol
aqueous ammonium ion, AH,° = -132.5 kJ/mol
%3D
3. Calculate the heat of reaction, AH, for the combustion of one mole of C,H6(1)
using the reactions provided below.
'rxn
6 C(s, graphite) + 3 H2(g) → C6H6(1) AH = 49.0 kJ
H2(g) + ½ O2(g) → H2O(I) AH = -285.8 kJ
C(s, graphite) + O2(g) → CO2(g) AH = -393.5 kJ
4. Calculate the heat of reaction, A Hxn, for the reaction between nitrogen and oxygen
to form nitrogen dioxide using the reactions provided below.
2 NH3(g)
N2(g) + 3 H2(g)
AH = 92.4 kJ
2 NO2(g) + 7 H2(g) → 2 NH3(g) + 4 H2O(1) AH=-1302.6 kJ
H,O(1) -
H2(g) + ½ O2(g)
AH = 285.8 kJ
75
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