Chemistry

Problem

28 g of

N_2

gas is contained in a flask at a pressure of 10 atm and at a temperature of

57^\circ\text{C}

. It is found that due to leakage in the flask, the pressure is reduced to half and the temperature to

27^\circ\text{C}

. The quantity of

N_2

gas that leaked out is a.

11/20

g b.

20/11

g c.

5/63

g d.

63/5

Intuitive explanation

The key is recognizing that the ideal gas law $PV = nRT$ connects pressure, moles, and temperature—and the flask volume stays constant. Calculate how many moles you started with, then use the new pressure and temperature to find how many moles remain. The difference tells you what leaked out. Since molar mass of $N_2$ is 28 g/mol, converting between moles and grams is straightforward.

Intuitive explanation

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