A 5.46 L cylinder contains 2.35 mol of helium gas at 7.0◦C. What is the pressure of the gas in the cylinder?
since PV/T = k,
you want P (in torr) such that
(P*5.46)/(7.0+273.15) = (760*2.35*22.4)/273.15
I got 7514.952712, is that correct?
7514.952712 what? lbs? tons? kilopascals?
I solved for P and got 7514.952712 torr.
To find the pressure of the gas in the cylinder, you can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure of gas (in Pascals)
V = Volume of gas (in liters)
n = Number of moles of gas
R = Ideal gas constant (0.0821 L·atm/(mol·K) or 8.314 J/(mol·K))
T = Temperature of gas (in Kelvin)
First, convert the given temperature from Celsius to Kelvin by adding 273.15:
T = 7.0 + 273.15 = 280.15 K
Now you have all the necessary values to plug into the ideal gas law equation.
P * V = n * R * T
Rearrange the equation to solve for P:
P = (n * R * T) / V
Plug in the values:
P = (2.35 mol * 0.0821 L·atm/(mol·K) * 280.15 K) / 5.46 L
P = 3.78 atm
Therefore, the pressure of the gas in the cylinder is 3.78 atm.