Ask Question
19 January, 23:07

Calculate the standard enthalpy of formation of carbon disulfide (CS2) from it's elements, given that C (graphite) + O2 (g) → CO2 (g) ΔH o rxn = - 393.5 kJ/mol S (rhombic) + O2 (g) → SO2 (g) ΔH o rxn = - 296.4 kJ/mol CS2 + 3O2 (g) → CO2 (g) + 2SO2 (g) ΔH o rxn = - 1073.6 kJ/mol

+2
Answers (1)
  1. 20 January, 02:16
    0
    Standard enthalpy of formation of Carbon disulfide CS2 = 87.3 KJ/mol

    Explanation:

    forming CS2 means that it should in the product side

    C (graphite) + O2 → CO2 ΔH = - 393.5

    2S (rhombic) + 2O2 → 2SO2 ΔH = - 296.4 x 2

    CO2 + 2SO2 → CS2 + 3O2 ΔH = - 1073.6 x - 1

    the second reaction is multiplied by 2 so that the SO2 and O2 can cancel out.

    the third reaction is reversed (multiplied by - 1) so that CS2 will be on the product side.

    after adding the reaction and cancelling out similarities, the final reaction is: C (graphite) + 2S (rhombic) → CS2

    Add ΔH to find the enthalpy of formation of CS2

    ΔHf = (-393.5) + (-296.4 x 2) + (-1073.6 x - 1) = 87.3 KJ/mol

    be aware of signs
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Calculate the standard enthalpy of formation of carbon disulfide (CS2) from it's elements, given that C (graphite) + O2 (g) → CO2 (g) ΔH o ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers