What is the volume occupied by 0.118 mol of helium gas at a pressure of 0.97atm and a temperature of 32 degrees celius? R=0.0821 L atm/mol K
Use PV = nRT
Don't forget to change T to Kelvin.
To find the volume of a gas, you 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, you need to convert the given values to the appropriate units. The pressure is already given in atm, but the temperature needs to be converted from Celsius to Kelvin. To do this, simply add 273.15 to the Celsius temperature:
T(K) = T(°C) + 273.15
In this case, the temperature is 32 degrees Celsius, so:
T(K) = 32 + 273.15 = 305.15 K
Now we can plug the values into the ideal gas law equation:
(0.97 atm) * V = (0.118 mol) * (0.0821 L atm/mol K) * (305.15 K)
Now, we can calculate the volume by rearranging the equation and solving for V:
V = (0.118 mol) * (0.0821 L atm/mol K) * (305.15 K) / (0.97 atm)
V ≈ 2.98 L
Therefore, the volume occupied by 0.118 mol of helium gas at a pressure of 0.97 atm and a temperature of 32 degrees Celsius is approximately 2.98 liters.