Several properties of gases can be experimentally measured: temperature, pressure, volume, and the amount of the gas (i.e., the number of moles). The ideal gas law states that the relationship between these properties, or variables, in a mathematical formula.
The ideal gas law is PV = nRT.
P is the pressure in atmospheres (atm), V is the volume in liters (L), n is the number of moles, R is the gas constant (0.0821 L∙atm/(mol∙K)), and T is the temperature in Kelvins (K).
Using the ideal gas law, determine the pressure of a 0.820 mole sample of oxygen gas, under a temperature of 25.0 °C and a volume of 4.78 L.
First, we need to convert the temperature from Celsius to Kelvin:
T (K) = 25.0 + 273.15 = 298.15 K
Now, we can rearrange the ideal gas law to solve for pressure:
P = nRT/V
Plugging in the values:
P = (0.820 mol)(0.0821 L∙atm/(mol∙K))(298.15 K) / 4.78 L
P = 20.97 atm
Therefore, the pressure of the 0.820 mole sample of oxygen gas is 20.97 atm.