00:02
How many grams of magnesium nitrate will be produced in the reaction when 31 grams of magnesium carbonate is combined with 13 grams of nitric acid? so this is a limiting reactant type of equation.
00:19
So what we're going to do is we're going to start with magnesium carbonate and we're going to convert those 31 grams to moles by dividing by.
00:31
The molar mass of 84 .314 grams.
00:37
From here we're going to convert magnesium carbonate into magnesium nitrate since that's what we're looking for.
00:46
But we're only going to convert the moles and this is a one -to -one ratio.
00:51
So for every one mole of magnesium carbonate you get one mole of magnesium nitrate.
00:59
Now eventually we're going to go to mass, but we're going to stop here at moles because the definition of limiting reactant is the reactant that produces the fewest number of moles of a specific product.
01:12
So we have to go to moles and then we'll convert those moles to mass.
01:18
So next, let's do nitric acid, where we have hn .o3.
01:24
And for that, we have 13 grams of that.
01:28
And we're going to convert it to moles, one mole over the molar mass of 63 .012 grams.
01:38
Next, for every one mole of magnesium nitrate, you're going to have or need two moles of nitric acid.
01:52
So here we have to divide by two because that's what's in the bottom.
01:56
So let's start with magnesium carbonate, where we have 31 divided by 84 .314.
02:03
Multiplied by 1, and that's going to be 0 .367 .67 moles.
02:13
And then for nitric acid, we have 13 .0 divided by 63 .012, and then divide that by 2, or multiply by 1 half, and we're going to have 0 .10315 moles, and both of these are of magnesium nitrate.
02:35
Now, first, we go to mass, so we're going to take 0 .10315 moles, and we're going to multiply this by the molar mass of magnesium nitrate, 148 .32 grams for every one mole...