```
PV = nRT
```
Where:
* P is the pressure in atmospheres
* V is the volume in liters
* n is the number of moles of gas
* R is the ideal gas constant (0.08206 L * atm / mol * K)
* T is the temperature in Kelvin
We are given the following information:
* n = 3.21 mol
* V = 56.2 L
* T = 44 °C + 273.15 = 317.15 K
* P = 793 torr * (1 atm / 760 torr) = 1.043 atm
We can rearrange the ideal gas law to solve for V:
```
V = nRT / P
```
Substituting our values in, we get:
```
V = (3.21 mol * 0.08206 L * atm / mol * K * 317.15 K) / 1.043 atm
```
```
V = 84.5 L
```
Therefore, the gas occupies 84.5 L at the given conditions.
