00:01
So the question says there is a one liter container, one liter container which has two gases in it, that is carbon monoxide and o2.
00:17
So these two gases are held at a temperature 1 .0 into 10 base to 3 kelvin.
00:26
We can write this value as 1 ,000 kelvin for further calculation.
00:34
And in this container, the pressure is 2 .2 atmosphere.
00:43
So this is at time t is equal to 0.
00:45
And after some time t, what happens is that the pressure drops from 2 .2 to 1 .9 atmosphere.
00:57
And this is due to the pressure drop is due to the formation of carbon monoxide in the container.
01:08
So from this data, we have asked to calculate the mass of co2 that is produced in terms of grams.
01:19
So how many grams of co2 has been produced? so from this, as a container contain carbon monoxide and oxygen, so we can write the formation of co2 gas as 2co plus o2 gives rise to 2co2.
01:40
This is what the reaction is happening in the container.
01:44
And we have also a formula that this number of moles is given by pv is equal to rt.
01:51
So this is the number of moles of gas.
01:55
Now we can write the initial number of moles of gas divided as p1 v1 divided by rt.
02:04
P1 is the initial pressure, which is 2 .2 atmosphere into volume is the 1 liter.
02:10
The container is 1 liter divided by r is a gas constant, which is constant value that is 0 .0821 into temperature given as 1 ,000.
02:22
So if we simplify this, it will come around 0 .0268 moles.
02:31
Now let's calculate the final number of moles...