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methanol can be utilized in a multitude of reactions. Consider the following reaction for the decomposition of methanol: 2CH3OH(f) → 2CH4(g) + 02(g) Use Hess' Law to calculate the enthalpy change (in kJ-mol·l) of this reaction, given the following known thermochemical data: H20(£) → /202(g) + H2(g) CHĄ(g) + H20(g) 2H2(g) + CO(g) → CH3OH(t) H20(g) → H20(f) AH, = 285.8 k] •mol-1 = 206.1 kJ · mol-1 ΔΗ = -128.3 kJ · mol- ΔΗ AH, = -44.00 kJ · mol-1 3H2(g) + CO(g)

methanol can be utilized in a multitude of reactions. Consider the following reaction for the decomposition of methanol: 2CH3OH(f) → 2CH4(g) + 02(g) Use Hess' Law to calculate the enthalpy change (in kJ-mol·l) of this reaction, given the following known thermochemical data: H20(£) → /202(g) + H2(g) CHĄ(g) + H20(g) 2H2(g) + CO(g) → CH3OH(t) H20(g) → H20(f) AH, = 285.8 k] •mol-1 = 206.1 kJ · mol-1 ΔΗ = -128.3 kJ · mol- ΔΗ AH, = -44.00 kJ · mol-1 3H2(g) + CO(g)

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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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: 2.1 2CH3ОН(?) — 2CH4(9) + 02(g) Use Hess' Law to calculate the enthalpy change (in kJ-mol-1) of this reaction, given the following known thermochemical data: H20(?) → 1/202(g) + H2 (g) CH4(g) + H,0(g) 2H-(9) + со(g) — сH;оН (0) H20(g) → H20(f) = 285.8 kJ · mol-1 = 206.1 kJ · mol-1 AH, → 3H2(g) + CO(g) CH3OH(?) ΔΗ ДН, — —128.3 k/ : тol-1 AH, = -44.00 kJ • mol-1 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-l)
Transcribed Image Text: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: 2.1 2CH3ОН(?) — 2CH4(9) + 02(g) Use Hess' Law to calculate the enthalpy change (in kJ-mol-1) of this reaction, given the following known thermochemical data: H20(?) → 1/202(g) + H2 (g) CH4(g) + H,0(g) 2H-(9) + со(g) — сH;оН (0) H20(g) → H20(f) = 285.8 kJ · mol-1 = 206.1 kJ · mol-1 AH, → 3H2(g) + CO(g) CH3OH(?) ΔΗ ДН, — —128.3 k/ : тol-1 AH, = -44.00 kJ • mol-1 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-l)
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