A 2.35-L container is filled with 165 g argon. If the pressure is 10.0 atm, what is the temperature?
To determine the temperature in this scenario, 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 find the number of moles of argon. We can use the molar mass of argon to convert the given mass to moles:
molar mass of argon = 39.95 g/mol
moles of argon = mass of argon / molar mass of argon
moles of argon = 165 g / 39.95 g/mol
Next, we can substitute the known values (pressure, volume, number of moles, and gas constant) into the ideal gas law equation and solve for the unknown temperature:
(10.0 atm) * (2.35 L) = (moles of argon) * (0.0821 L·atm/(mol·K)) * T
Simplifying:
23.5 L·atm = (moles of argon) * (0.0821 L·atm/(mol·K)) * T
Finally, solve for T:
T = (23.5 L·atm) / ((moles of argon) * (0.0821 L·atm/(mol·K)))
Substitute the value for moles of argon that we calculated earlier to get the final answer.