Carbon disulfide is a colorless liquid. When pure, it is nearly odorless, but the commercial product smells vile. Carbon disulfide is used in the manufacture of rayon and cellophane. The liquid burns as follows: CS2(l) + 3O2(g) → CO2(g) + 2SO2(g)Calculate the standard enthalpy change for this reaction usingstandard enthalpies of formation.

Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as [tex]\Delta H^o[/tex]

The equation used to calculate enthalpy change is of a reaction is:

[tex]\Delta H^o_{rxn}=\sum [n\times \Delta H^o_f(product)]-\sum [n\times \Delta H^o_f(reactant)][/tex]

For the given chemical reaction:

[tex]CS_2(l)+3O_2(g)\rightarrow CO_2(g)+2SO_2(g)[/tex]

The equation for the enthalpy change of the above reaction is:

[tex]\Delta H^o_{rxn}=[(1\times \Delta H^o_f_{(CO_2)})+(2\times \Delta H^o_f_{(SO_2)})]-[(1\times \Delta H^o_f_{(CS_2)})+(3\times \Delta H^o_f_{(O_2)})][/tex]

We are given:

[tex]\Delta H^o_f_{(CO_2)}=-393.52kJ/mol\\\Delta H^o_{SO_2}=-296.8kJ/mol\\\Delta H^o_f_{(O_2)}=0kJ/mol\\\Delta H^o_{CS_2}=89.70kJ/mol[/tex]

Putting values in above equation, we get:

[tex]\Delta H^o_{rxn}=[(1\times (-393.52))+(2\times (-296.8))]-[(1\times (89.70))+(3\times (0)]\\\\\Delta H^o_{rxn}=-1076.82kJ[/tex]

Hence, the standard enthalpy change of the reaction is -1076.82kJ