What is QV in chemistry?
Subsequently, one may also ask, what is the relationship between QP and QV?
qp vs. qv. I want to make sure that my understanding of heat at constant temperature versus constant pressure is correct. Thus, at constant pressure: ΔUp=qp-PΔV; at constant volume: ΔUv=qv (work doesn't exist at constant volume) and, finally, at constant pressure: ΔH=ΔU+PΔV.
Subsequently, question is, what does Δhrxn mean? ΔHrxn, or the change in enthalpy of a reaction, has the same value of ΔH as in a thermochemical equation, but is in units of kJ/mol being that it is the enthalpy change per moles of any particular substance in the equation.
Also know, is QP a state function?
qp. Work is a state property as it is directly proportional to the object's distance moved against the opposing force and this distance depends on the path taken. Since deltaU = W + q, and work is a state function, it seems that the heat given off must be dependent on the path as well.
How do you define enthalpy?
Enthalpy is a thermodynamic property of a system. It is the sum of the internal energy added to the product of the pressure and volume of the system. It reflects the capacity to do non-mechanical work and the capacity to release heat. Enthalpy is denoted as H; specific enthalpy denoted as h.