Question

Argon gas behaves as an ideal gas at normal temperatures. Consider a 5.00 L tank filled with Argon at room temperature (25.0 °C) and 10 atmospheres. (R = 0.08206 L·atm/mol·K)

How many moles of Argon are in the tank?

Answer 1

We can use the ideal gas law to solve this problem:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

We need to convert the temperature to Kelvin by adding 273.15:

T = 25.0 + 273.15 = 298.15 K

Substituting the values:

(10 atm) (5.00 L) = n (0.08206 L·atm/mol·K) (298.15 K)

Simplifying:

n = (10 atm) (5.00 L) / (0.08206 L·atm/mol·K) (298.15 K)

n = 20.4 mol

Therefore, there are 20.4 moles of Argon in the tank.