posted by lyan on .
Q6) A 10 L container contains a mixture of 0.8 g of He and 8 g of Ar at 0 oC.
a) (1 pt) Calculate the total pressure of the gas mixture.
b) (1 pt) Calculate the partial pressure of each gas in the gas mixture.
c) (1 pt) If the initial total pressure of the container was 1.5 atm (at 0 oC), what will be the new pressure if the container is heated to 100 oC (Volume is kept constant)?
d) (1 pt) If the initial total pressure of the container was 1.5 atm (with 0.8 g He + 8 g Ar), what will be the new pressure in the container if 1 mol of Ne is added to this gas mixture
(Volume is kept constant).
a. Convert g He and g Ar to moles. mols = g/molar mass. Add moles and use total moles and PV = nRT to solve for total P.
b. Use PV = nRT and individual n values for partial pressure of each gas.
c.(P1/T1) = (P2/T2)
d. sum n He + n Ar + 1 mol for Ne. Then PV = nRT