50 liters cylinder is filled with Ar gas to a pressure of 10130KPa at 30C. How many moles of At gas are in the cylinder
PV = nRT and solve for n.
P = given in kPa.
V = 50 L
n = solve
R = 8.314
T = 273 + 30 = ?
You may also convert kPa given to atm by dividing by 101.325 kPa.
If you do that then R must be in L*atm/mol*K and that is 0.08206
To find the number of moles of Ar gas in the cylinder, you can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in Pa)
V = Volume (in m^3)
n = Number of moles
R = Gas constant (8.314 J/(mol·K))
T = Temperature (in Kelvin)
Let's convert the given values into appropriate units first:
Pressure: 10130 kPa = 10130,000 Pa
Volume: 50 liters = 0.05 m^3
Temperature: 30°C = 30 + 273.15 K = 303.15 K
Now, you can substitute these values into the ideal gas law equation to find the number of moles (n):
(10130,000 Pa) * (0.05 m^3) = n * (8.314 J/(mol·K)) * (303.15 K)
Simplifying the equation:
n = (10130,000 Pa * 0.05 m^3) / (8.314 J/(mol·K) * 303.15 K)
n = 162.47 moles
Therefore, there are approximately 162.47 moles of Ar gas in the cylinder.