If 21.5 mol of an ideal gas is at 4.81 atm at 91.60 ∘C, what is the volume of the gas?
PV/T is constant, so you want
4.81V/(91.60+273.15) = 1*(21.5*22.4)/273.15
Thanks!
To find the volume of an ideal gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in liters)
n = Number of moles
R = Ideal gas constant (0.0821 L·atm/(mol·K))
T = Temperature (in Kelvin)
First, we need to convert the Celsius temperature to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 91.60°C + 273.15 = 364.75 K
Now, we can use the given values and the ideal gas law equation to find the volume:
PV = nRT
V = (nRT) / P
Substituting the given values:
V = (21.5 mol * 0.0821 L·atm/(mol·K) * 364.75 K) / 4.81 atm
Simplifying the equation:
V = (21.5 * 0.0821 * 364.75) / 4.81
V ≈ 390.89 L
Therefore, the volume of the gas is approximately 390.89 liters.