00:01
Today, we have an equation where hydrogen sulfide gas reacts with dioxygen gas to produce sulfur dioxide and water vapor.
00:09
And this reaction is occurring at 0 .5 atmospheres of pressure, at a rate of 629 liters per second, and at a temperature of 184 degrees celsius.
00:20
And what we want to know is the rate of sulfur dioxide production in kilograms per second.
00:26
So the first step in solving this is we have to balance our equation.
00:30
And right now, there are more oxygens in the products than the reactants.
00:36
So we balance this out by writing a three here.
00:38
But now there's more oxygen in the reactants.
00:42
So we write a two here and a two here.
00:45
And now both sides are balanced in terms of oxygens.
00:48
However, now there's more hydrogens in the products than the reactants.
00:52
So we write a two here.
00:54
And now the number of elements matches on both sides, the reactants and the products.
00:58
Now we have to calculate the number of moles of sulfur dioxide this reaction is producing.
01:05
And we do this by using the ideal gas law equation pv equals n rt.
01:13
Now in this equation, n equals the number of moles...