4. Use the pressure of the butane gas (your answer from question #3 above), along with the temperature and volume recorded in the lab, to determine the moles of butane gas collected in the lab. You will use the ideal gas law (and the ideal gas constant, R) for this calculation; just make sure that all of the measurements have the correct units necessary for the calculation.
temp=297 k volume=90 ml
To determine the moles of butane gas collected in the lab, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the butane gas
V = volume of the gas
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/K·mol)
T = temperature in Kelvin
First, let's make sure all the measurements are in the correct units for the calculation. The pressure should be in atm, the volume in liters, and the temperature in Kelvin.
Given:
Pressure (P) = answer from question 3 (in atm)
Volume (V) = 90 mL = 0.09 L (conversion: 1 L = 1000 mL)
Temperature (T) = 297 K (already in Kelvin)
Now, we can rearrange the ideal gas law equation to solve for moles (n):
n = PV / RT
Substituting the given values:
n = (P * V) / (R * T)
Plugging in the values we have:
n = (P * 0.09) / (0.0821 * 297)
Now, you can substitute the value of pressure (from question 3) into this equation to calculate the moles of butane gas collected in the lab.