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When 1 mole of H2CO(g) reacts with O2(g) to form CO2(g) and H2O(l) according to the following equation, 563 kJ of energy are evolved. H2CO(g) + O2(g)CO2(g) + H2O(l) Is this reaction endothermic or exothermic? What is the value of q? Write a balanced thermochemical equation

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Answer:

This is an exothermic reaction

q = 563 kJ

Explanation:

Step 1: The balanced thermochemical equation

H2CO(g) + O2(g) → CO2(g) + H2O(l)        ΔH = -563 kJ

This is a combustion, this means there will be released heat. This means it's an exothermic reaction.

The energy involved, will be released (that's why ΔH is negative)

q has the same value as ΔH (but positive)

q = 563 kJ