How many moles of oxygen gas must be in a 12.2 L container to exert a pressure of 0.877 atm at a temperature of 35.0°C (the ideal gas constant in this case is 0.0821 L atm / mole K)?
PV=nRT
n=PV/RT temps in kelvins.
To find the number of moles of oxygen gas in the container, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P is the pressure of the gas in atmospheres (0.877 atm)
V is the volume of the container in liters (12.2 L)
n is the number of moles of gas we want to find
R is the ideal gas constant (0.0821 L atm / mole K)
T is the temperature of the gas in Kelvin (35.0°C + 273.15 = 308.15 K)
Rearranging the equation to solve for n, the number of moles:
n = PV / RT
n = (0.877 atm * 12.2 L) / (0.0821 L atm / mole K * 308.15 K)
n ≈ 5.12 moles
Therefore, there must be approximately 5.12 moles of oxygen gas in the 12.2 L container to exert a pressure of 0.877 atm at a temperature of 35.0°C.