 Okay, let's do this problem together. It says ammonia and sulfuric acid to react to form ammonium sulfate write an equation for the reaction Okay, so that's the first part of this problem So you have to know what these things are. So Ammonia is NH3 and I'm going to put it in the gaseous form And then I'm going to react that with sulfuric acid And we're also just going to put that in the gaseous form So we can think of this as kind of like a high-temperature reaction And that's going to form What ammonium sulfate? So the ammonium ion is NH4 plus, okay And the sulfate ion is SO4 2 minus So ammonium sulfate Is NH4 2 SO4 But if you look at that, right, how many nitrogens do we have here? Two. On this side, we only have one, right? So in order to balance this equation We're going to have to put it two bit, okay? So the second part of this problem says Determine the starting mass and grams of each reactive 20 grams of ammonium sulfate is produced So the mass of ammonium sulfate is 20.3 grams And The mass of sulfuric acid remaining is 5.89 grams So the starting mass of each reactive Okay, so this tells us That ammonia was the limiting reaction Why? Because there's still Sulfuric acid left over So that means the amount of Ammonium sulfate came directly from the amount of ammonia, okay So let's just figure out what I'm talking about So the mass of ammonium sulfate is 20 0.3 grams so NH4 2 SO4 So I want to figure out the number of moles So so I can use the balance reaction So the number of moles of ammonium sulfate, okay? So in order to do that I'm going to have to use the Periodic table to figure out the molar mass of ammonium sulfate So let's do that together Periodic table over here 4 is 8 1.08 32.07 Plus 4 times 16 So I got 1.32.15 That's the molar mass of 1.32.15 grams of ammonium Sulfate on the bottom one mole Ammonium sulfate on the top so that gives me the number of moles of ammonium sulfate So what am I looking for? I'm looking for the mass of the three starting materials not the number of moles of the product, right? so Let's figure out well What is the number of moles of ammonium? Because that's the limiting reagent that we will be able to find from this Okay, well, can I get that through the balance reaction equation? Can I get it? So how many moles of ammonium sulfate to moles of ammonium? Well 1 to 2 But So is that what we wanted? The number of moles of ammonium? No, we wanted the what? The mass, yeah, the grams So What do we do? Well, we're gonna have to figure out well, what's the molar mass of ammonium? 14.01 Plus 3 times 1.08 which is 17.03 grams per mole So the bottom down here 1 mole and h3 17.03 grams and h3 And that should does give us the mass of ammonium, right? So that's how much of ammonium we started out. So let's figure that out. So 20.3 divided by 132.15 times 2 times 17.0 So the mass of ammonium that we started with 5.23 grams of ammonium So well, what's the mass of sulfuric acid that we started with? Well, we're going to have to figure out the number of moles of ammonium and then use the reaction equation again, okay? So what we can do is take this number and divide it by 17.03 and we'll get the number of moles of ammonium, right? Now let's just write that out So mass of sulfuric acid is going to be equal 5.23 grams of ammonium 17.03 grams of ammonium just going backwards one step Okay, that's going to cancel the fact Now we're using the reaction equation again to do this to this Okay, so for every two moles of ammonium We've got one mole of sulfuric acid And we want to know the mass of sulfuric acid So we're going to have to figure out what the molar mass of sulfuric acid Okay, so the molar mass of sulfuric acid 2 times 1.008 plus 32.07 plus 4 times 16 So 98.7 from being trying I should give us the number of grams of sulfuric acid So 5.23 divided by 17.03 divided by 2 multiplied by 98.09 So that 15.03 So 15.1 grams of sulfuric acid All right, but it said that the mass of sulfuric acid that we have left over was 5.89 Right, so the mass total so this would be the mass that was reacted So the mass total of sulfuric acid equal the mass reacted plus the mass left over so we got 15.11 plus 5.89 grams 1.0 grams of sulfuric acid So the two numbers Should we kill it