A sample of 2.0 moles of helium gas is contained in a tank with a volume of 5.0 Lat a temperature of 25°C. What is the pressure of the gas in the tank in atm?

Answer 1

To solve this problem, we can use the ideal gas law equation:

PV = nRT

where:
P is the pressure of the gas
V is the volume of the gas
n is the number of moles of gas
R is the ideal gas constant (0.0821 L.atm/mol.K)
T is the temperature of the gas in Kelvin

First, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273
T(K) = 25 + 273
T(K) = 298 K

Now we can substitute the given values into the ideal gas law equation:
P(5.0 L) = (2.0 mol)(0.0821 L.atm/mol.K)(298 K)
P(5.0 L) = 49.88 atm

Therefore, the pressure of the gas in the tank is 49.88 atm.