When H2S(g) reacts with O2(g) according to the following reaction, 518 kJ of energy are evolved for each mole of H2S(g) that reacts. Complete the following thermochemical equation.

Question

When H₂S(g) reacts with O₂(g) according to the following reaction, 518 kJ of energy are evolved for each mole of H₂S(g) that reacts. Complete the following thermochemical equation.

2H₂S(g) + 3O₂(g) --> 2H₂O(g) + 2SO₂(g) | deltaH = _____kJ

Answer 1

Evolved is a way of saying given off so if this energy is given off for 1 mole of H2S, the energy would have to be doubled for 2 moles: So you would have: 518kJ x2= 1036kJ.