# Problem: Dinitrogen difluoride gas is collected at -17.0°C in an evacuated flask with a measured volume of 30.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.260 atm. Calculate the mass and number of moles of dinitrogen difluoride gas that were collected.

###### FREE Expert Solution

We’re being asked to calculate the mass and number of moles of dinitrogen difluoride (N2F2) gas that were collected.

We’re going to calculate the moles of N2F2 using the ideal gas equation.

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K

Given:

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###### Problem Details

Dinitrogen difluoride gas is collected at -17.0°C in an evacuated flask with a measured volume of 30.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.260 atm. Calculate the mass and number of moles of dinitrogen difluoride gas that were collected.

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Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.