2.1Methanol is an attractive fuel source in a sustainable, green economy. The chemical energy inherent inmethanol can be utilized in a multitude of reactions. Consider the following reaction for the formationof methanol:2CH,(g) + 0,(9) → 2CH,OH(f)Use Hess' Law to caleculate the enthalpy change (in kJ-mol") of this reaction, given the followingknown 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) · molAH, = 571.6 k/ molAH, = -128.3 k) mol-Methanol can also be combusted in the presence of oxygen in order to release its energy. 5.24 g ofmethanol was placed in a bomb calorimeter (with a known heat capacity of 0.874 kJ-K"), together with2.50 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

Answered: Image /qna-images/answer/63ef1f6b-60e7-4cde-866b-555812675b40.jpg

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, (9) + 0,(9) – 2CH,0H(f) Use Hess' Law to calculate the enthalpy change (in kJ-mot") of this reaction, given the following known thermochemical data: H,0(?) – H,0(g) CH, (9) + H,0(g) – 3H,(g) + CO(g) 2H,0(f) – 0,(g) + 2H;(g) 2H, (g) + CO(g) - CH,OH(?) AH, = 44.00 k) - mol AH, = 206.1 k) - mol AH, = 571.6 kj - mol AH, = -128.3 k) - mol-

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, (9) + 0,(9) – 2CH,0H(f) Use Hess' Law to calculate the enthalpy change (in kJ-mot") of this reaction, given the following known thermochemical data: H,0(?) – H,0(g) CH, (9) + H,0(g) – 3H,(g) + CO(g) 2H,0(f) – 0,(g) + 2H;(g) 2H, (g) + CO(g) - CH,OH(?) AH, = 44.00 k) - mol AH, = 206.1 k) - mol AH, = 571.6 kj - mol AH, = -128.3 k) - mol-

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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