Use heat of formation data to determine ?H for the combustion of hydrogen sulfid

Question

Use heat of formation data to determine ?H for the combustion of hydrogen sulfide according to the following reaction: 2 H2S(g) + 3 O2(g) ? 2 SO2(g) + 2 H2O(?) ?H = ? ?Hfo for compounds: H2S(g) is -20.15 kJ/mol , SO2(g) is -296.4 kJ/mol , H2O(?) is -285.8 kJ/mol

Explanation / Answer

FOLLOW THIS rst, switch the first rxn around... SO2 + H2O--> H2S + 3/2 02 new DHrxn = +563kJ then multiply it by two 2 SO2 + 2 H2O --> 2 H2S + 3 02 DHrxn = 1126kJ then combine the two reactions, canceling as necessary 2 SO2 + 2 H2O --> 2 H2S + 3 02 DHrxn = 1126kJ CS2 + 3 O2 --> CO2 + 2 SO2 DHrxn = -1075kJ (the 2 SO2 and 3 O2 will be canceled out) so you're left with: CS2 + 2 H20 --> 2 H2S + CO2 therefore DHrxn = 1126 + -1075 = 51kJ

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