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.