Answer:
A. Partial pressure of krypton, Kr is 346.97 mmHg
B. Partial pressure of nitrogen, N2 is 364.03 mmHg.
Step-by-step explanation:
Step 1:
Data obtained from the question. This include the following:
Total pressure (Pt) = 711 mmHg
Mass of Kr = 11.7 g
Mass of N2 = 4.10 g
Partial pressure of Kr =..?
Partial pressure of N2 =...?
Step 2:
Determination of the number of mole of krypton, Kr and nitrogen, N2. This is illustrated below:
Molar mass of Kr = 84g/mol
Mass of Kr = 11.7g
Mole of Kr =?
Mole = mass /Molar mass
Mole of Kr = 11.7/84 = 0.139 mole
Molar mass of N2 = 2x14 = 28g/mol
Mass of N2 = 4.10g
Mole of N2 =?
Mole = mass /Molar mass
Mole of N2 = 4.1/28 = 0.146 mole
Step 3:
Determination of the mole fraction for each gas. This is illustrated below:
Mole of Kr = 0.139 mole
Mole of N2 = 0.146 mole
Total mole = 0.139 + 0.146 = 0.285 mole
Mole fraction of Kr = mol of Kr/total mol
Mole fraction of Kr = 0.139/0.285
Mole fraction of Kr = 0.488
Mole fraction of N2 = mol of N2/total mol
Mole fraction of N2 = 0.146/0.285
Mole fraction of N2 = 0.512
A. Determination of the partial pressure of krypton, Kr.
This is illustrated below:
Total pressure (Pt) = 711 mmHg
Mole fraction of Kr = 0.488
Partial pressure of Kr =..?
Partial pressure = mole fraction x total pressure
Partial pressure of Kr = 0.488 x 711
Partial pressure of Kr = 346.97 mmHg
B. Determination of the partial pressure of nitrogen, N2
This is illustrated below:
Total pressure (Pt) = 711 mmHg
Mole fraction of N2 = 0.512
Partial pressure of N2 =?
Partial pressure = mole fraction x total pressure
Partial pressure of N2 = 0.512 x 711
Partial pressure of N2 = 364.03 mmHg