The partial pressure of CH4(g) is 0.185 atm and that of O2(g) is 0.300 atm in a mixture of the two gases.
a) What is the mole fraction of each gas in the mixture?
b) If the mixture occupies a volume of 11.5 L at 65 degress C, calculate the total number of moles of gas in the mixture.
a) partial pressure CH4 = 0.185 atm.
partial pressure O2 = 0.300
total pressure = 0.185 + 0.300
X=mol fraction CH4 = pressure CH4/total pressure.
X=mol fraction O2 = pressure O2/total pressure.
b)Use PV = nRT
Use total P, you have V, n is what you solve for, R is the gas constant (0.08205 L*atm/mol*K) and T is 65 (don't forget to change to Kelvin). Using total pressure will get total n.
.201
To find the mole fraction of each gas in the mixture, we need to calculate the partial pressure of each gas and the total pressure of the mixture.
a)
The partial pressure of CH4(g) is given as 0.185 atm.
The partial pressure of O2(g) is given as 0.300 atm.
To find the total pressure of the mixture, we simply add the partial pressures of the two gases:
Total pressure = 0.185 atm + 0.300 atm = 0.485 atm
Now, we can find the mole fraction of each gas in the mixture using the formula:
Mole fraction = Partial pressure of the gas / Total pressure
For CH4:
Mole fraction of CH4 = 0.185 atm / 0.485 atm = 0.381
For O2:
Mole fraction of O2 = 0.300 atm / 0.485 atm = 0.619
Therefore, the mole fraction of CH4 is 0.381 and the mole fraction of O2 is 0.619.
b)
To calculate the total number of moles of gas in the mixture, we can use the ideal gas law equation PV = nRT, where P is the total pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
Given:
Pressure (P) = 0.485 atm
Volume (V) = 11.5 L
Temperature (T) = 65 degrees C = 65 + 273.15 K = 338.15 K
Gas constant (R) = 0.08205 L*atm/mol*K
We can rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT
Plugging in the values, we get:
n = (0.485 atm) * (11.5 L) / (0.08205 L*atm/mol*K * 338.15 K)
Calculating this expression, we get the total number of moles in the mixture.