A tank at is filled with of chlorine pentafluoride gas and of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. chlorine pentafluoride mole fraction: partial pressure: dinitrogen difluoride mole fraction: partial pressure: Total pressure in tank:

A 8.00 L tank at 26.9 C is filled with 17.3 g of sulfur hexafluoride gas and 5.53 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank.

a) Mole fraction of sulfur hexafluoride = 0.59

Mole fraction of dinitrogen difluoride = 0.41

b) partial pressure of sulfur hexafluoride = 0.365 atm

partial pressure of dinitrogen difluoride = 0.254

c) Total pressure = 0.619atm

Explanation:

To calculate the moles :

Total moles = 0.118 + 0.083 = 0.201

According to ideal gas equation:

P = pressure of gas = ?

V = Volume of gas = 8.00 L

n = number of moles = 0.201

R = gas constant =

T = temperature =

n+h→nh3

we must remember that nitrogen and hydrogen are both diatomic molecules in their standard gas form. this adjusts the equation to

n2+h2→nh3

now we need to adjust coefficients in order to balance the atoms on each side of the equation. currently we have 2 atoms of nitrogen and 2 atoms of hydrogen on the reactant side and 1 atom of nitrogen and 3 atoms of hydrogen on the product side.

we can balance the hydrogens by placing a coefficient of 2 in front of ammonia and a coefficient of 3 in front of the hydrogen.

n2+3h2→2nh3

this gives us 6 hydrogen on each side and coincidentally the nitrogens now equal 2 on each side.

take a better picture and ill do it