Dinitrogen difluoride gas is collected at in an evacuated flask with a measured volume of. When all the gas has been collected, the pressure in the flask is measured to be. Calculate the mass and number of moles of dinitrogen difluoride gas that were collected. Be sure your answer has the correct number of significant digits.

0.175 mol; 11.6 g

Explanation:

There is some info missing. I think this is the original question.

Dinitrogen difluoride gas is collected at 22.0 °C in an evacuated flask with a measured volume of 25.0L. When all the gas has been collected, the pressure in the flask is measured to be 0.170atm. Calculate the mass and number of moles of dinitrogen difluoride gas that were collected. Be sure your answer has the correct number of significant digits.

Given data

Temperature (T) = 22.0°C + 273.15 = 295.2 K

Volume (V) = 25.0 L

Pressure (P) = 0.170 atm

We can find the moles of N₂F₂ using the ideal gas equation.

P * V = n * R * T

0.170 atm * 25.0 L = n * (0.08206 atm. L/mol. K) * 295.2 K

n = 0.175 mol

The molar mass of N₂F₂ is 66.01 g/mol. The mass of N₂F₂ is:

0.175 mol * (66.01 g/mol) = 11.6 g