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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Chemistry

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23 February, 06:45

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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Zaiden Terry · Answer 1

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