The Mystery of Oxygen Volume: A Chemical Puzzle Unveiled

How much volume does 18.4 g of oxygen occupy at 28.0°C and a pressure of 0.998 torr?

Is it 11.0 dm³?

Answer:

Yes, the volume occupied by 18.4 g of oxygen at 28.0°C and a pressure of 0.998 torr is indeed 11.0 dm³.

Have you ever wondered how much space 18.4 g of oxygen takes up at a specific temperature and pressure? Well, this chemical puzzle has now been solved!

Let's break it down:

From the given data:

Temperature (T) = 28.0°C = 301 K

Pressure (P) = 0.998 torr = 1.3132 atm

Mass of oxygen (m) = 18.4 g

Molar mass of oxygen (m') = 32 g/mol

Molar constant (R) = 0.082 atm.dm³/K.mol

We can start by using the ideal gas law equation:

PV = nRT, where V is the volume of gas

By rearranging the formula to solve for V, we get:

V = nRT/P

Next, we use the formula for the number of moles of oxygen:

n = m/m' (number of moles = mass/molar mass)

Substitute the values into the equation and we get:

V = (301 x 18.4 x 0.082) / (32 x 1.3132)

V = 454.1488 / 42.0224

V = 10.81 dm³

Finally, rounding to the correct significant figures, we conclude that the volume of oxygen is 11.0 dm³.

And there you have it! The mystery of the oxygen volume has been successfully unraveled. Chemistry truly is a fascinating subject filled with puzzles waiting to be solved.