# Problem: 4.00-L flask contains nitrogen gas at 25 °C and 1.00 atm pressure. What is the final pressure in the flask if an additional 2.00 g of N2 gas is added to the flask and the flask cooled to -55°C?

###### FREE Expert Solution

Step 1. Calculate the number of moles of gas intially present in the container 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

Step 2. Calculate the total number of moles with added gas.
Step 3. Calculate the new pressure.

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###### Problem Details

4.00-L flask contains nitrogen gas at 25 °C and 1.00 atm pressure. What is the final pressure in the flask if an additional 2.00 g of N2 gas is added to the flask and the flask cooled to -55°C?