If 63.5 moles of an ideal gas is at 4.03 atm at 51.80 °C, what is the volume of the gas?
Use PV = nRT
would I do 4.03*51.80
No, What do you not understand? T must be in kelvin
P is pressure in atmospheres.
V = volume in L
n = mols
R = ideal gas constant
T = temperture in kelvin (273.15 +|C = K)
To determine the volume of a gas, we can use the ideal gas law equation. The ideal gas law states that:
PV = nRT
Where:
P = Pressure (in atmospheres)
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 given temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature.
T = 51.80 °C + 273.15 = 324.95 K
Now we can plug in the values we have into the ideal gas law equation and solve for V:
PV = nRT
V = (nRT) / P
V = (63.5 mol * 0.0821 L·atm/mol·K * 324.95 K) / 4.03 atm
Calculating this expression will give us the volume of the gas in liters.