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 amount of gas, in moles, of a 8.32 L sample of hydrogen gas, under a temperature of 310 K and a pressure of 1.7 atm.
First, we will rearrange the ideal gas law equation to solve for n (number of moles):
PV = nRT
n = PV / RT
Given:
P = 1.7 atm
V = 8.32 L
R = 0.0821 L∙atm/(mol∙K)
T = 310 K
Plugging in the values:
n = (1.7 atm * 8.32 L) / (0.0821 L∙atm/(mol∙K) * 310 K)
n = 14.144 / 25.442
n = 0.556 moles
Therefore, there are 0.556 moles of hydrogen gas in the 8.32 L sample under the given conditions.