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2.2 Methanol can also be combusted in the presence of oxygen in order to release its energy. 5.24 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 0.874 kJ-K), together with 2.50 kg water. After methanol was combusted, the temperature of the water increased by 10.3 °C. Calculate the change in internal energy of methanol (in kJ-mol")

2.2 Methanol can also be combusted in the presence of oxygen in order to release its energy. 5.24 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 0.874 kJ-K), together with 2.50 kg water. After methanol was combusted, the temperature of the water increased by 10.3 °C. Calculate the change in internal energy of methanol (in kJ-mol")

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.147QP: The head of a strike anywhere match contains tetraphosphorus trisulfide, P4S3. In an experiment, a...
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2.1 Methanol is an attractive fuel source in a sustainable, green economy. The chemical energy inherent in methanol can be utilized in a multitude of reactions. Consider the following reaction for the formation of methanol: 2CH,(g) + 0,(9) → 2CH,OH(f) Use Hess' Law to caleculate the enthalpy change (in kJ-mol") of this reaction, given the following known thermochemical data: H,0(?) – H,0(g) CH, (9) + H,0(g) 3H,(9) + CO(9) 2H,0(e) – 0,(g) + 2H2(g) 2H, (9) + Co(g) - CH,OH(?) AH, = 44.00 kJ mol- AH, = 206.1 k) · mol AH, = 571.6 k/ mol AH, = -128.3 k) mol- Methanol can also be combusted in the presence of oxygen in order to release its energy. 5.24 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 0.874 kJ-K"), together with 2.50 kg water. After methanol was combusted, the temperature of the water increased by 10.3 °C. Calculate the change in internal energy of methanol (in kJ-mol") 2.2
Transcribed Image Text:2.1 Methanol is an attractive fuel source in a sustainable, green economy. The chemical energy inherent in methanol can be utilized in a multitude of reactions. Consider the following reaction for the formation of methanol: 2CH,(g) + 0,(9) → 2CH,OH(f) Use Hess' Law to caleculate the enthalpy change (in kJ-mol") of this reaction, given the following known thermochemical data: H,0(?) – H,0(g) CH, (9) + H,0(g) 3H,(9) + CO(9) 2H,0(e) – 0,(g) + 2H2(g) 2H, (9) + Co(g) - CH,OH(?) AH, = 44.00 kJ mol- AH, = 206.1 k) · mol AH, = 571.6 k/ mol AH, = -128.3 k) mol- Methanol can also be combusted in the presence of oxygen in order to release its energy. 5.24 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 0.874 kJ-K"), together with 2.50 kg water. After methanol was combusted, the temperature of the water increased by 10.3 °C. Calculate the change in internal energy of methanol (in kJ-mol") 2.2
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