What volume does a mixture of 14.2 g of He and 21.6 g of H2 occupy at 28 degrees celcius and 0.985 atm?
PV=nRT n= moles of HE + moles H2
think about that. If you have studied Dalton's Law of Partial Pressures, it makes perfect sense...each gas has a partial pressure, and the sum of them is .985atm
To find the volume of the mixture of He and H2, we need to 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 calculate the number of moles for each gas using their respective masses and molar masses:
For helium (He):
Molar mass of He = 4 g/mol
Number of moles of He = mass of He (in grams) / molar mass of He
For hydrogen (H2):
Molar mass of H2 = 2 g/mol
Number of moles of H2 = mass of H2 (in grams) / molar mass of H2
Next, we need to convert the temperature from Celsius to Kelvin:
Temperature in Kelvin = 28°C + 273.15
Now we can solve for the volume:
V = (nHe + nH2)RT / P
Substituting the values into the equation, we have:
V = [(mass of He / molar mass of He) + (mass of H2 / molar mass of H2)] * R * (temperature in Kelvin) / pressure
Calculating the masses of He and H2, and substituting the values into the equation, we can find the volume.