Question

1. A mixture of krypton and oxygen gases, in a 5.61 L flask at 64 °C, contains 8.22 grams of krypton and 9.52 grams of oxygen. The

partial pressure of oxygen in the flask is ____ atm and the total pressure in the flask is
___ atm.

2. A mixture of xenon and oxygen gases, in a 6.50 L flask at 27 °C, contains 22.3 grams of xenon and 1.70 grams of oxygen. The partial pressure of oxygen in the flask is
____ atm and the total pressure in the flask is ____

Answer 1

To find the partial pressure of gases in a mixture, convert the temperature to Kelvin, calculate the moles of each gas using their molar masses, and apply the ideal gas law to determine each gas's partial pressure. The total pressure is the sum of the partial pressures. Follow the same steps for any mixtures, adjusting for molar masses and temperatures accordingly.

Step-by-step explanation:

To calculate the partial pressure of gases, you’ll need to use the ideal gas law in combination with Dalton's Law of Partial Pressures. Dalton's law states that the total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases in the mixture. The ideal gas law is represented by PV=nRT, which relates pressure (P), volume (V), number of moles (n), the gas constant (R), and temperature (T).

First, convert the temperature from Celsius to Kelvin by adding 273.15. Next, calculate the number of moles of each gas using their respective molar masses (Kr = 83.798 g/mol, O2 = 32.00 g/mol).

Once you have the moles of each gas, you can find each gas's partial pressure by rearranging the ideal gas law to solve for P (P = nRT/V). After finding the partial pressures, the total pressure of the mixture is the sum of the individual partial pressures.

For the mixture of xenon and oxygen gases, follow the same steps, using the molar mass of xenon (Xe = 131.293 g/mol). Remember to adjust the temperature to Kelvin as well.