Question

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

Answer 1

The reaction where 1 mole of H2CO(g) reacts with O2(g) to form CO2(g) and H2O(l) is exothermic, evolving -563 kJ of energy. This is represented in the balanced thermochemical equation with a negative enthalpy change (ΔH = -563 kJ).

Step-by-step explanation:

When 1 mole of H2CO(g) reacts with O2(g) to form CO2(g) and H2O(l), the reaction is exothermic because energy is released. The value of q in this context represents the amount of energy evolved during the reaction, which is -563 kJ (negative sign indicates energy is released by the system). Therefore, the balanced thermochemical equation incorporating the heat of reaction would be as follows:

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

An exothermic reaction is characterized by the release of energy to the surroundings, with a negative enthalpy change (ΔH), indicating that the products are at a lower energy level than the reactants. Conversely, an endothermic reaction absorbs energy, with a positive enthalpy change, indicating that the products are at a higher energy level than the reactants.

Answer 2

This is an exothermic reaction

q = 563 kJ

Step-by-step 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