00:01
Hello everyone.
00:02
Here in this question, a reaction is given in which iron oxide react with carbon monoxide to form iron and carbon dioxide.
00:13
Now the amount of iron oxide used in this reaction is 22 .15 grams and the amount of carbon monoxide used is 15 .98 grams.
00:25
Now we have to determine the amount of excess reactant left after completion of the reaction.
00:34
To determine the excess reactant, we have to determine the limiting reagent in the reaction.
00:41
For determining the limiting reagent, let us determine the number of moles of iron oxide and carbon monoxide used in the reaction.
00:50
So the number of moles of iron oxide is equal to the weight of iron oxide is equal to the weight of iron oxide used in reaction divided by its molecular weight.
01:13
Let's put the values.
01:15
We know that weight of the iron oxide used in reaction is 22 .15 and its molecular weight is 1 .5.
01:23
159 .69 .69.
01:27
After calculating, we get that here, 0 .138 moles of iron oxide is used in the reaction.
01:41
Similarly, let's determine the number of moles of carbon monoxide used in the reaction.
01:51
It is also calculated in similar way.
01:54
The weight of carbon monoxide used in reaction divided by its molecular weight.
02:01
Weight of carbon monoxide used in reaction is 15 .98 and its molecular weight is 28.
02:11
So this comes out that the number of moles of carbon monoxide is 0 .5707 moles.
02:23
Now, as from the reaction, we can see that 1 mole of iron oxide react with 3 moles of carbon monoxide.
02:43
So, 0 .138 moles of iron oxide must react with 3 multiplied by 0 .138 moles of iron oxide must react with 3 multiplied by 0 .138...