2 one of the results of acid rain is the reaction of...

One of the results of acid rain is the reaction of sulfuric acid, H2SO4, with calcium carbonate, CaCO3, to produce calcium sulfate, CaSO4, and carbonic acid, H2CO3. The chemical equation for this reaction is: H2SO4 + CaCO3 = CaSO4 + H2CO3 A student demonstrates the reaction by mixing 25.00 g of H2SO4 with 25.00 g of CaCO3. a. How many moles of each reactant does the student mix? b. Identify the limiting reactant. Explain how you know this. c. Calculate the theoretical mass of the excess reactant. d. Soon after mixing the reactants, the student determines that 33.17 g of CaSO4 was produced by the reaction. Is this a reasonable result? Show calculations to defend your answer.

Transcript

00:01 So today, we're given the reaction for acid rain where sulfuric acid h2s .o .4 combines with calcium carbonate, caco3, to produce calcium sulfate, caso4, and carbonic acid, h2co3.

00:17 We're told that to demonstrate this, a student reacts 25 grams of sulfuric acid and 25 grams of calcium carbonate.

00:26 We're first asked to calculate how many moles this is.

00:29 So for our sulfuric acid, we'll take our 25 grams that are given, and then we'll cancel out grams by using grams in our dimensional analysis.

00:41 So we put the molar mass of one mole of sulfuric acid on the bottom, which is 98 .08 grams.

00:51 And this gives us 0 .255 moles of sulfuric acid.

01:00 Now, for our calcium carbonate, we will put, again, are given 25 grams, and we'll cancel this out by using the number of moles in one, or the number of grams in one mole of calcium carbonate, which is 100 .09 grams, and this gives us 0 .250 moles.

01:29 All right? and then we're asked to identify the limiting reagent.

01:33 So let's look at our reaction.

01:35 All right? we see that one mole of sulfuric acid reacts with one mole of calcium carbonate.

01:43 And since we have less calcium carbonate, that means that it's our limiting reagent because not all of this sulfuric acid can react.

01:52 So the calcium carbonate is the limiting reagent because there's less of it and they react in a one -to -one mole ratio.

02:03 Now for the theoretical mass of the excess reagent, we're left with about 0 .005 moles of sulfuric acid as excess, and this is about 0 .490 grams of sulfuric acid...

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