Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is th
ID: 738954 • Letter: C
Question
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 35.0 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 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?
H = kJ
(e) Calculate E when 665.0 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 HopHelpCh5N1
Explanation / Answer
CH3OH(g) -> CO(g) + 2H2(g) Change in H= +90.7 kJ (a) If the enthalpy change is 19.0 kJ, how many grams of hydrogen gas are produced? (in g) 19kJ @ (2 mol H2)(@2.02g/mol) / 90.7 kJ = 0.8463 g H2 your answer(3sigfigs): 0.846 g H2 ======================================… (c) How many kilojoules of heat are released when 25.0 g of CO(g) reacts completely with H2 (g) to form CH2OH(g) at constant pressure. (in kJ) this reverse reaction has the reverse energy: CO(g) + 2H2(g) --> CH3OH(g) Change in H= - 90.7 kJ 25.0 g CO @ (-90.7kJ) / (1mol CO)(@28.01 g/mol) = - 80.953 kJ kyour answer(3sigfigs): 81.0 kJ are released