Consider the following reaction.CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ(a) the reaction is endothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.answer isH = 113.23 kJ (c) If the enthalpy change is 17.0 kJ, how many grams of hydrogen gas are produced? answer is .757 g (d) How many kilojoules of heat are released when 14.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure? answer isH = -45.3 kJ (e) Calculate delta E when 500.0 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 ???? I've already tried 85.7, 1624, and 1614. I am so lost
Consider the following reaction.CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ(a) the reaction is endothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.answer isH = 113.23 kJ (c) If the enthalpy change is 17.0 kJ, how many grams of hydrogen gas are produced? answer is .757 g (d) How many kilojoules of heat are released when 14.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure? answer isH = -45.3 kJ (e) Calculate delta E when 500.0 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 ???? I've already tried 85.7, 1624, and 1614. I am so lost
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