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Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ-K-'), together with 2.50 kg water. 2.2 After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in internal energy of methanol (in kJ-mol-')

Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ-K-'), together with 2.50 kg water. 2.2 After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in internal energy of methanol (in kJ-mol-')

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 89GQ: Chloroform, CHCl3, is formed from methane and chlorine in the following reaction. CH4(g) + 3 Cl2(g) ...
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Please answer 2.2 Only. 

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 decomposition of methanol: 2CH;OH(f) → 2CH4(g) + 02(g) Use Hess' Law to calculate the enthalpy change (in kJ-mol-1) of this reaction, given the following known thermochemical data: H20(?) → /202(g) + H2(g) CH4(g) + H20(g)→ 3H2(g) + CO(g) 2H2 (g) + CO(g) → CH3OH(?) H20(g) → H20(t) ДН, — 285.8 k] -тol-1 ДН, — 206.1 k] :тol-1 ΔΗ ДН, 3D —128.3 k) : тol-1 ΔΗ Дн, 3D — 44.00 k] -тol-1 [5] 2.2 Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ.K-'), together with 2.50 kg water. After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in internal energy of methanol (in kJ-mol-') [5]
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 decomposition of methanol: 2CH;OH(f) → 2CH4(g) + 02(g) Use Hess' Law to calculate the enthalpy change (in kJ-mol-1) of this reaction, given the following known thermochemical data: H20(?) → /202(g) + H2(g) CH4(g) + H20(g)→ 3H2(g) + CO(g) 2H2 (g) + CO(g) → CH3OH(?) H20(g) → H20(t) ДН, — 285.8 k] -тol-1 ДН, — 206.1 k] :тol-1 ΔΗ ДН, 3D —128.3 k) : тol-1 ΔΗ Дн, 3D — 44.00 k] -тol-1 [5] 2.2 Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ.K-'), together with 2.50 kg water. After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in internal energy of methanol (in kJ-mol-') [5]
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