Answer :
The question is about thermochemistry, specifically heat exchange at constant pressure (qp) and constant volume (qv). In the provided reaction, although there's a change in the number of moles due to hydrogen gas formation, since the gas likely moves out freely, keeping the pressure constant, therefore qp ≈ qv.
This question is dealing with the topic of thermochemistry, specifically the heat exchange at constant pressure (qp) or constant volume (qv). Normally, these are not equal because some heat can be used to do work under constant pressure conditions. However, since this is a chemical reaction in a solution, the volume usually does not change. Hence, in this context, qp should be approximately equal to qv.
In general, for gases, if we assume all gases are ideal and if the number of moles of gas is not changing (no gases are being produced or consumed), then we have qp = qv. Here, there is a change in the number of moles due to the formation of hydrogen gas, which could make qp different from qv. However, the gas is likely to move freely out of the solution because it isn't contained, so the pressure remains constant and the volume change doesn't contribute to the work done. Thus, still, qp ≈ qv.
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