Consider the combustion of liquid methanol, CH3OH(l):CH3OH(l) + 3/2O2(g)----> CO2(g) + 2 H2O(l) ΔH = -726.5 kJ(a) What is the enthalpy change for the reverse reaction?(b) Balance the forward reaction with whole-number coefficients.What is ΔH for the reaction represented by thisequation? (c) Which is more likely to be thermodynamicallyfavored, the forward reaction or the reverse reaction?(d) If the reaction were written to produce H2O(g) insteadof H2O(l), would you expect the magnitude of ΔH to increase,decrease, or stay the same? Explain.
Consider the combustion of liquid methanol, CH3OH(l):CH3OH(l) + 3/2O2(g)----> CO2(g) + 2 H2O(l) ΔH = -726.5 kJ(a) What is the enthalpy change for the reverse reaction?(b) Balance the forward reaction with whole-number coefficients.What is ΔH for the reaction represented by thisequation? (c) Which is more likely to be thermodynamicallyfavored, the forward reaction or the reverse reaction?(d) If the reaction were written to produce H2O(g) insteadof H2O(l), would you expect the magnitude of ΔH to increase,decrease, or stay the same? Explain.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 96QRT
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Consider the combustion of liquid methanol, CH3OH(l):
CH3OH(l) + 3/2O2(g)----> CO2(g) + 2 H2O(l) ΔH = -726.5 kJ
(a) What is the enthalpy change for the reverse reaction?
(b) Balance the forward reaction with whole-number coefficients.
What is ΔH for the reaction represented by this
equation? (c) Which is more likely to be thermodynamically
favored, the forward reaction or the reverse reaction?
(d) If the reaction were written to produce H2O(g) instead
of H2O(l), would you expect the magnitude of ΔH to increase,
decrease, or stay the same? Explain.
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