Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is th
ID: 737156 • 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?
A)exothermic
B)endothermic
(b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.
H =___ kJ
(c) If the enthalpy change is 13.0 kJ, how many grams of hydrogen gas are produced?
______g
(d) How many kilojoules of heat are released when 12.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?
H = ____kJ
(e) Calculate E when 825.0 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
a)since H is positive the reaction is endo thermic... b)for 1 mole of CH3OH (i.e 32g) 90.7kJ are transferred for 40 g heat transferred is=90.7*40/32=113.375KJ c)for 90.7KJ 2 moles (4 g)of hydrogen is released so h2 gas released=13*4/90.7=0.573g d)reverse reation is exothermic with H=-90.7KJ so heat released=-90.7*12.5/28=-38.87KJ so H=-38.87KJ