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?

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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?

(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?

(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  kJ

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