Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic (b) Calculate the amount of heat transferred when 55.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. H = kJ (c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g (d) How many kilojoules of heat are released when 12.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure? H = kJ
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic (b) Calculate the amount of heat transferred when 55.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. H = kJ (c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g (d) How many kilojoules of heat are released when 12.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure? H = kJ
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Consider the following reaction.
CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ
(a) Is the reaction exothermic or endothermic?
exothermic
endothermic
(b) Calculate the amount of heat transferred when 55.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.
H = kJ
(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced?
g
(d) How many kilojoules of heat are released when 12.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?
H = kJ
(e) Calculate E when 450.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K
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