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H can be viewed as a system's enthalpy, or its total internal energy. While this energy often takes the form of heat, this is not always the case. It can apply to other forms of energy as well. Since H represents energy, delta H represents the change in this energy over the course of a chemical reaction. Delta H naught represents this change at standard conditions, as based on the conditions the reaction undergoes, the delta H value can change. Q represents solely heat energy, as it is directly related to the heat capacity of a substance, or the amount of heat energy that must be put into a substance to increase its temperature. As for Qp, I am not sure, but it is likely a derivative of Q, which represents heat energy.
As the above comment says, delta H represents the change of energy in a reaction from its final state to its initial state, regardless of the path it took to get there. q is the heat given off by a system during a reaction, and its sign will tell us whether the reaction is exothermic (negative value) or endothermic (positive value), similarly to delta H. qp will be the same as q and delta H (an expression of heat and/or energy) but in a reaction where pressure is held constant, as denoted by the “p.”
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