Dalton s law of Partial Pressure and Mole I-ructions (P_lotal = p_1 + p_2 + p_3,
ID: 955223 • Letter: D
Question
Dalton s law of Partial Pressure and Mole I-ructions (P_lotal = p_1 + p_2 + p_3, +... and X_1 = n_1/n_tota1 and p_1 = X_1 P_ytotal where X_1 is the mole fraction of gas 1, n_1 is the # of moles of gas is the total # of moles in the gas mixture, p, is the partial pressure of gas 1, and P_total is the total pressure) If a sample of oxygen gas is collected over water at a pressure of 0.921 atm and 23degreeC, what is the partial pressure of the oxygen gas? A mixture of gases exerting a pressure of 1.11 atm consists of 0.20 mol of O: gas, 0.3 mol of H: gas, and 0.7 mol of CO_2 gas. What is the partial pressure of the O_2 gas, the H_2 gas and the CO_2 gas? 0.5 mol of O_2 is added to a cylinder containing 0.7 mol of H_2 at 0.6 atm. What is the mole fraction of each gas? What is the partial pressure of O_2 and the total pressure of the cylinder? A 150 mL flask was evacuated (all air removed) and into it was forced 50. mL of I I_2 gas under a pressure of 750 torr; 75 mL of Ar under a pressure of 450 torr; and 100. mL of O_2 under a pressure of 350 torr. Determine the partial pressure (in torr) of each of the gases in the 150 mL flask and determine the total pressure of the gas mixture. (See problem #4) The pressure of a sample of nitrogen gas and water vapor is 947 torr at 20degreeC. What is the partial pressure of nitrogen?Explanation / Answer
16 ) partial pressure = x1Ptotal
pratial pressure of oxygen gas = 16/18 [0.921] = 0.818 atm
17) total pressure = PO2 +PH2+PCO2
partial pressure O2 = X1Ptotal =[ 0.2 / 1.2 ] * 1.11atm = 0.185 atm
partial pressure H2 = [0.3 / 1.2 ] * 1.11 atm = 0.2775 atm
partial pressure CO2 = [ 0.7/1.2] * 1.11 atm = 0.6475 atm
18) mol fraction of O2 = 0.5 / 1.2 = 0.416
mol fraction of H2 = 0.7/1.2 = 0.583
partial pressure of O2 = [0.5/0.7] * 0.6 atm = 0.428 atm
total pressure = 0.428 + 0.6 = 1.028 atm
19 ) partial pressure in 150 ml flask H2 = [50/150] * 750 torr = 250 torr
partial pressure in 150 ml flask Ar = [75/150] * 450 torr = 225 torr
partial pressure in 150 ml flask O2 = [100/150] * 300 =200 torr
total pressure = P1 +P2+P3 = 675 torr
20) partial pressure of nitrogen gas = [14/32] * 947 torr = 414 torr
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