Question

The thermochemical equation for the combustion of one mole of carbon monoxide is as follows: CO(g) + ½ O2 → CO2(g) ΔH = −283 kJ Calculate the heat change for the decomposition of 2.00 lb carbon dioxide gas into CO and oxygen.

Answer 1

given equation is

CO_(g) + 1/2 O_2(g)     CO_2(g)   H = -283 KJ

write above equation in revese manner

CO_2(g)         CO_(g) + 1/2 O_2(g)   H = + 283 KJ

1 lb = 453.592 gm then 2 lb = 907.184 gm

molar mass of CO₂ = 44.01 gm / mole then 907.184 gm of CO₂ = 907.184 / 44.01 = 20.613 mole of CO₂

According to reaction for 1 mole of CO₂ conversion to CO and oxygen H = 283 KJ then for 20.613 mole of CO₂

H = 283 20.613 = 5833.479 KJ

heat change for the decomposition of 2.00 lb carbon dioxide into CO and oxygen = 5833.479 KJ