How do you use the equation for heat flow at constant temperature and pressure (latent heat of fusion or vaporization)? #q = nDeltaH#
The equation you're referring to is
This equation is used to establish a relationship between how much heat is involved when a number of moles of a substance undergoes a phase change.
Let's say, for example, that you want to know how much heat is needed to melt 3 moles of ice at its melting temperature of
The equation will look like this
In water's case, the molar enthalpy of fusion is equal to 6.02 kJ/mol. This means that, in order to convert 1 mole of solid ice at
If you want to know how much heat would be needed to convert 3 moles of ice at its melting point to liquid water, you'd have
Here's another example. Let's say that you need to determine how much heat is released when 5 moles of water condense from steam at
Notice that the equation has a negative sign this time. This is used to show that heat is released, not absorbed, when condensation occurs.
The molar enthalpy of vaporization will tell you how much energy is absorbed when 1 mole of liquid water is converted to 1 mole of steam. In water's case,
This means that you release 40.7 kJ for every mole of water that goes from steam at
This time, you have
Converting that many moles of water from steam to liquid would release that much heat.
As a conclusion, you need to remember that this equation uses number of moles, not grams, and that it can only be used for phase changes, since they take place at constant temperature.
Just a note about phase changes: they occur at a constant temperature, but the pressure can change (but it doesn't have to).
When you say
...so that the units match. For example, molar enthalpy
You may not have learned this explicitly yet, but a way of defining
You can also see this here.
The result of working with this equation is as follows (dropping the subscripts):
Thus, if the pressure is constant (like a normal day, really)...
Basically, the idea of this is that when you are in General Chemistry, those teachers/professors purposefully do not tell you that you are working under constant pressure because it is supposed to be self-evident, usually, and it is also irrelevant to the problem because that's all you're working with at the time. You're working at a constant altitude, so the pressure tends to not change unless you induce a change.
You may have also encountered something in General Chemistry that is similar:
where the standard enthalpy of reaction is basically a "normalization" of the heat transfer that occurs while using a certain number of