Question

a 7.00 l tank at -7.8 is filled with of chlorine pentafluoride gas and of carbon dioxide gas. you can assume both gases behave as ideal gases under these conditions. calculate the mole fraction of each gas. round each of your answers to significant digits.

Answer 1

To calculate the mole fraction of each gas in the tank, you can use the ideal gas law equation PV = nRT. Rearrange the equation to solve for n, the number of moles. Then, use the moles of each gas to calculate the mole fraction by dividing the moles of each gas by the sum of the moles of both gases.

Step-by-step explanation:

To calculate the mole fraction of each gas, we first need to determine the moles of each gas. We can use the ideal gas law equation: PV = nRT. Rearranging the equation, we have n = PV/RT, where n is the number of moles, P is the pressure, V is the volume, R is the ideal gas constant, and T is the temperature in Kelvin.

Given that the initial volume of the tank is 7.00 L, the mole fraction of chlorine pentafluoride gas can be calculated as the moles of chlorine pentafluoride divided by the total moles of gas in the tank. The mole fraction of carbon dioxide gas can be calculated similarly. The mole fractions will be the ratio of moles of each gas divided by the sum of the moles of both gases.

For example:

Mole fraction of chlorine pentafluoride = (moles of chlorine pentafluoride)/(moles of chlorine pentafluoride + moles of carbon dioxide)

Mole fraction of carbon dioxide = (moles of carbon dioxide)/(moles of chlorine pentafluoride + moles of carbon dioxide)

Remember to convert the temperature from Celsius to Kelvin by adding 273.15.