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What is the pressure in a 13.0- L cylinder filled with 36.6 g of oxygen gas at a temperature of 319 K ?

Answer :

Final answer:

To find the pressure, we apply the Ideal Gas Law, PV=nRT. For that, we first convert the given mass of oxygen to moles, then substitute the values along with the ideal gas constant into the Ideal Gas Law equation. Upon calculating, the pressure is found to be about 2.28 atm.

Explanation:

In order to find the pressure in this scenario, we must use the Ideal Gas Law which is stated as PV=nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. Here, the volume V is 13.0 L and the temperature T is 319 K. But we're also given the mass of the gas and not the moles. So, we need to convert the mass to moles using the molar mass of oxygen, which is 32.00 g/mol.

First, let's convert the given mass of oxygen to moles. Moles = mass/molar mass = 36.6 g / 32.00 g/mol =~ 1.14 moles

Now, we can substitute these values into the Ideal Gas Law equation along with the ideal gas constant R (which is 0.0821 L·atm/mol·K) to solve for pressure: P = nRT/V = (1.14 mol)(0.0821 L·atm/K·mol)(319 K)/ 13.0 L

By calculating the above, the pressure is found to be ≈ 2.28 atm.

Learn more about Ideal Gas Law here:

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