Question

A sample of neon gas collected at a pressure of 584 mm Hg and a temperature of 296 K has a mass of 21.8 grams. The volume of the sample is

Answer 1

Solving for V, we get V = (1.08 mol x 0.0821 L·atm/mol·K x 296 K) / 0.768 atm = 32.8 L. Please check the explanation below to help you remember the steps.

Step-by-step explanation:

To find the volume of the gas, we can use the ideal gas law equation, which is PV = nRT.

First, we need to convert the pressure from mm Hg to atm because the ideal gas law uses atm. The conversion factor is 1 atm = 760 mm Hg. So, 584 mm Hg = 584/760 = 0.768 atm.

Next, we need to find the number of moles (n) of the gas. We know that the molar mass of neon (Ne) is approximately 20.18 g/mol. So, 21.8 g of Ne = 21.8/20.18 = 1.08 mol.

The value of R (the ideal gas constant) is 0.0821 L·atm/mol·K.

Now we can substitute these values into the ideal gas law equation:

0.768 atm x V = 1.08 mol x 0.0821 L·atm/mol·K x 296 K

Solving for V, we get V = (1.08 mol x 0.0821 L·atm/mol·K x 296 K) / 0.768 atm = 32.8 L.