What is the δg for the following reaction at 25°c? so3 (g) h2o (l) → h2so4 (l) given: so3 (g) : δg = - 368 kjper mole h2o (l) : δg = - 237 kj per mole h2so4 (l) : δg = - 689.9 kj per mole

Question

Sampson

Chemistry

1 January, 23:17

What is the δg for the following reaction at 25°c? so3 (g) h2o (l) → h2so4 (l) given: so3 (g) : δg = - 368 kjper mole h2o (l) : δg = - 237 kj per mole h2so4 (l) : δg = - 689.9 kj per mole

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Deegan Payne · Answer 1

We are given with the equation that produces sulfuric acid from the reaction of sulfur trioxide gas and water. This is expressed in the balanced equation: SO3 + H2O = H2SO4. The enthalpy of the reaction in an aqueous solution can be determined by taking the difference between the summation of enthalpies of the products multiplied to their respective stoichiometric coefficient and the summation of enthalpies of the reactants multiplied to their respective stoichiometric coefficient. Answer is - 689.9 - (-368-237) equal to - 84.9 kJ per mole.