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2. The industrial method currently used to produce butanol is the hydration of butene. C,Ha(g) + H,O(g) →> CH,„O(g) The enthalpy values for the following reactions are: 4C(s) + 4H,(g) → CHo(g) 4C(s) + 5H,(g) + ½0,(g) → C,H„O(g) 2H,(g) + O,(g) → 2H,0(g) AH = -7-1 kJ mo–1 AH = - 292-8 kJ mol–1 AΗ=-483-6 kl mol-1 Using the data above, calculate the enthalpy change, in kJ mol-1, to produce butanol by hydration of butene.

2. The industrial method currently used to produce butanol is the hydration of butene. C,Ha(g) + H,O(g) →> CH,„O(g) The enthalpy values for the following reactions are: 4C(s) + 4H,(g) → CHo(g) 4C(s) + 5H,(g) + ½0,(g) → C,H„O(g) 2H,(g) + O,(g) → 2H,0(g) AH = -7-1 kJ mo–1 AH = - 292-8 kJ mol–1 AΗ=-483-6 kl mol-1 Using the data above, calculate the enthalpy change, in kJ mol-1, to produce butanol by hydration of butene.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
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 36PS: Acetic acid. CH3CO2H, is made industrially by the reaction of methanol and carbon monoxide. CH3OH ()...
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2. The industrial method currently used to produce butanol is the hydration of butene. CHolg) + H,O(g) → CHz„O(g) The enthalpy values for the following reactions are: 4C(s) + 4H,(g) → CHa(g) 4C(s) + 5H,(g) + ½0;(g) → C,H,„O(g) 2H,(g) + O,(g) → 2H,0(g) AH = - 7:1 kJ mol-1 AH = - 292-8 kJ mol-1 AH = - 483-6 kJ mol-1 Using the data above, calculate the enthalpy change, in kJ mol-1, to produce butanol by hydration of butene. Calculation
Transcribed Image Text:2. The industrial method currently used to produce butanol is the hydration of butene. CHolg) + H,O(g) → CHz„O(g) The enthalpy values for the following reactions are: 4C(s) + 4H,(g) → CHa(g) 4C(s) + 5H,(g) + ½0;(g) → C,H,„O(g) 2H,(g) + O,(g) → 2H,0(g) AH = - 7:1 kJ mol-1 AH = - 292-8 kJ mol-1 AH = - 483-6 kJ mol-1 Using the data above, calculate the enthalpy change, in kJ mol-1, to produce butanol by hydration of butene. Calculation
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