Question

What is the partial pressure of chlorine gas, in mmHg, at 0.00 degrees Celsius and 1 atm in a gaseous mixture containing 46.5% nitrogen, 12.7% neon, 40.8% chlorine, by mass?

a) 407.5 mmHg
b) 562.4 mmHg
c) 619.2 mmHg
d) 738.1 mmHg

Answer 1

To find the partial pressure of chlorine gas, we need to calculate the moles of each gas in the mixture and then use the mole fraction to find the partial pressure. The partial pressure of chlorine gas is approximately 407 mmHg.

Step-by-step explanation:

To find the partial pressure of chlorine gas, we need to calculate the moles of each gas present. From the given percentages by mass, assume we have 100g of the mixture. This means we have 46.5g of nitrogen, 12.7g of neon, and 40.8g of chlorine.

Next, we calculate the moles of each gas using the molar masses. The molar mass of nitrogen is 28.01 g/mol, neon is 20.18 g/mol, and chlorine is 70.91 g/mol. Therefore, we have 1.664 mol of nitrogen, 0.629 mol of neon, and 0.576 mol of chlorine.

Finally, to find the partial pressure of chlorine gas, we can use the following equation:

Partial pressure of Cl2 = (Moles of Cl2 / Total moles) * Total pressure

Partial pressure of Cl2 = (0.576 mol / (1.664 mol + 0.629 mol + 0.576 mol)) * 1 atm = 0.407 atm = 407 mmHg