00:01
We're told that we have a reaction between ammonia and hydrogen sulfide, right, an equilibrium reaction in our product.
00:08
We have carbon sulfide and hydrogen gas.
00:17
And you just have to make sure that the equation is balanced.
00:22
Right.
00:23
Quite important that you make sure that the equation is balanced.
00:26
And you can rightly see that the equation is definitely not balanced.
00:29
Right.
00:29
Because if you have two modes of this here, right, so you need to have four modes of that here.
00:37
That is the balance equation.
00:39
Now, you were given the volume of the vessel, 8 .5 litres.
00:47
And we're told at equilibrium, we're given the concentrations.
00:53
Right.
00:54
So we're given the equilibrium.
00:56
At equilibrium, it is found that you had 4 .17 times 10 to the power of minus 4 molar methane, 0 .00751 molar hydrogen sulfide and the number of moles of and the equilibrium concentration of hydrogen gas.
01:15
And then you're asked, what is the equilibrium concentration of carbon sulfide if the chemical equilibrium content is 3 .57? well, so the kc expression for this would be the concentration of carbon sulfide, right, times the concentration of hydrogen gas, raised to the power of 4, divided by the concentration of methane, concentration of methane times the concentration of hydrogen sulfide squared...