Question

Given:

C(s) + O2(g) ---> CO2(g) ΔH = −393.5 kJ/mol

S(s) + O2(g) ---> SO2(g) ΔH = −296.8 kJ/mol

C(s) + 2S(s) ---> CS2(ℓ) ΔH = +87.9 kJ/mol

A) Calculate the standard enthalpy change for the following reaction CS2(ℓ) + 3O2(g) ---> CO2(g) + 2SO2(g)

ΔH° rxn = -1075 kJ/mol

B) Using the equation and standard enthalpy change for the reaction (from part A), calculate the amount of heat produced or consumed when 3.2 mol of CS2 reacts with excess O2. [ Select ]

Answer 1

\Delta{H}_{reaction}=\sum{\Delta{H_{products}-\sum\Delta{H}_{reactants}}}=-393.5+2(-296.8)-87.9=-1075kJ/molΔHreaction=∑ΔHproducts−∑ΔHreactants=−393.5+2(−296.8)−87.9=−1075kJ/mol

 

Answer: -1075 kJ/mol