Answer :

The pressure of 1.64 g of nitrogen gas confined to a volume of 0.280 L at 22 ∘C is 10.5 atm.

To solve this problem, we need to use the ideal gas law equation, which is PV=nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature. First, we need to calculate the number of moles of nitrogen gas using the formula n = m/M, where m is the mass of the gas and M is the molar mass of nitrogen gas.

m = 1.64 g
M = 28.0 g/mol (molar mass of nitrogen gas)

n = m/M = 1.64 g / 28.0 g/mol = 0.0586 mol

Next, we can plug in the values we have into the ideal gas law equation and solve for pressure:

P = nRT/V

P = (0.0586 mol) (0.0821 L·atm/mol·K) (295 K) / 0.280 L

P = 10.5 atm

Therefore, the pressure of 1.64 g of nitrogen gas confined to a volume of 0.280 L at 22 ∘C is 10.5 atm.

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