00:02
First, i will explain you the mechanism of the reaction that took place in this experiment.
00:08
Normally, the process in which hydrogen peroxide or your h202 breakdown and turns into oxygen and also water happens very slowly.
00:20
But it can be faster if we add a catalyst.
00:25
So, this is an organism that contains a special chemical called a catalyst.
00:32
That can act as a catalyst to help break down hydrogen peroxide, the corresponding chemical equation, which is two moles of your h202, yields to two moles of your h2o plus oxygen.
00:48
So in this part, we need to have a sample collected contains, not just oxygen, because it's a mixture of a small amount of water vapor and oxygen.
01:00
Then we can apply the dalton's law of partial pressure, which states that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the individual component gases at the same temperature.
01:15
We know that the total pressure in the room pressure, which is 1 .0 .atm, that is 760 mmhg, and the pressure of water vapor at 19 .6 degrees celsius, is 2 .23684 times 10 raised the power of negative 2 atm.
01:40
And this is a value available in the corresponding table.
01:43
And you could approximate this class data to 2 .24 times 10 raised the power of negative 2 atm, which will not greatly affect the results.
01:54
So we have the net expression to calculate the partial pressure of the oxygen.
01:59
So the total pressure, which is equals to the partial pressure of oxygen plus the water vapor.
02:07
So we have the total pressure minus the pressure of the water vapor.
02:17
So this would be 1 .0 atm minus 2 .24 times 10 raised par of negative 2 atm...