Answer :
The reaction absorbs energy, indicating that it is an endothermic reaction. The value of q for this reaction is +46.5 kJ.
This reaction involves the conversion of 2 moles of CO₂(g) and H₂(g) to C₂H₂(g) and H₂O(g) as represented by the balanced chemical equation: 2 CO₂(g) + 5H₂(g) → C₂H₂(g) + 4H₂O(g). Given that 46.5 kJ of energy are absorbed during this reaction, we can determine whether it is endothermic or exothermic and the value of q.
A reaction is considered endothermic if it absorbs energy from the surroundings, causing an increase in the internal energy of the system. Conversely, a reaction is exothermic if it releases energy to the surroundings, leading to a decrease in the system's internal energy.
In this case, the reaction absorbs 46.5 kJ of energy, indicating that it is an endothermic reaction. As a result, the internal energy of the system increases.
The value of q, which represents the heat absorbed or released during the reaction, can be determined using the given information. Since the reaction is endothermic and absorbs 46.5 kJ of energy, the value of q is positive. Therefore, the value of q for this reaction is +46.5 kJ.
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