10.0 grams of helium gas is pumped into a 2.55 L container. If the temperature of the gas is 34.0 °C, what is the pressure, in atmospheres?

P = 24.7 atm

Explanation:

Given data:

mass of helium = 10.0 g

Volume of container = 2.55 L

Temperature of gas = 34.0 °C (34.0 +273 = 307K)

Pressure of gas = ?

Solution:

Number of moles of helium:

Number of moles = mass/molar mass

Number of moles = 10.0 g/ 4 g/mol

Number of moles = 2.5 mol

Now we will determine the pressure of gas.

PV = nRT

P × 2.55 L = 2.5 mol × 0.0821 atm.L/mol.K × 307 K

P = 63.0 atm. L /2.55 L

P = 24.7 atm

c most likely

hop this let me know if it is wrong

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