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5. Given the equation for the combustion of one mole of CH.(g): CH(g) + 5/2 0,(g) à 2 CO,(g) + H,O(1) (a) Calculate the heat of combustion of C,H.(g) from the following data: (i) C,H (g) ® C,H(g) + 2 H,(g) DH = +311.4 kJ (ii) H,(g) + ½ O,(g) ® H¸O(1) DH =-285.9 kJ (iii) 2 CO,(g) + 3H,O(1) ® C,H(g) + 7/2 0,(g) DH = +849 kJ (b) Calculate the internal energy change, DE (in kJ), when 5.300 g of CH(g) was burned in excess oxygen at 45°C. R = 8.314 J/mol-K

5. Given the equation for the combustion of one mole of CH.(g): CH(g) + 5/2 0,(g) à 2 CO,(g) + H,O(1) (a) Calculate the heat of combustion of C,H.(g) from the following data: (i) C,H (g) ® C,H(g) + 2 H,(g) DH = +311.4 kJ (ii) H,(g) + ½ O,(g) ® H¸O(1) DH =-285.9 kJ (iii) 2 CO,(g) + 3H,O(1) ® C,H(g) + 7/2 0,(g) DH = +849 kJ (b) Calculate the internal energy change, DE (in kJ), when 5.300 g of CH(g) was burned in excess oxygen at 45°C. R = 8.314 J/mol-K

Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter15: Energy And Chemical Change
Section: Chapter Questions
Problem 112A: sample of natural gas is analyzed and found to be88.4% methane (CH4) and 11.6% ethane (C2H6) bymass....
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5. Given the equation for the combustion of one mole of CH.(g): СH(9) + 5/2 0,(g) a 2 СO (g) + НО) (a) Calculate the heat of combustion of C,H,(g) from the following data: (i) C,H (g) ® C¸H,(g) + 2 H,(g) DH = +311.4 kJ (ii) H,(g) + ½ 0,(g) ® H,O(1) DH =-285.9 kJ (iii) 2 CO,(g) + 3H,O(1) ® C̟H.(g) + 7/2 O,(g) DH = +849 kJ (b) Calculate the internal energy change, DE (in kJ), when 5.300 g of C,H.(g) was burned in excess oxygen at 45°C. R = 8.314 J/mol-K
Transcribed Image Text:5. Given the equation for the combustion of one mole of CH.(g): СH(9) + 5/2 0,(g) a 2 СO (g) + НО) (a) Calculate the heat of combustion of C,H,(g) from the following data: (i) C,H (g) ® C¸H,(g) + 2 H,(g) DH = +311.4 kJ (ii) H,(g) + ½ 0,(g) ® H,O(1) DH =-285.9 kJ (iii) 2 CO,(g) + 3H,O(1) ® C̟H.(g) + 7/2 O,(g) DH = +849 kJ (b) Calculate the internal energy change, DE (in kJ), when 5.300 g of C,H.(g) was burned in excess oxygen at 45°C. R = 8.314 J/mol-K
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