4. (4 points) When aluminum sulfide reacts with water, both...

4. (4 points) When aluminum sulfide reacts with water, both aluminum hydroxide and hydrogen sulfide are formed. ___ Al2S3 (s) + ___ H2O (l) ? ___ Al(OH)3 (s) + ___ H2S (g) a. Balance the reaction. b. What mass of water is required to completely react with 52.34 g of Al2S3? c. What mass of H2S and Al(OH)3 would be formed from the 52.34 g of Al2S3? 5. (2 points) How many grams of Fe can be harvested from 10.5 kg of Fe2O3 by the reaction with excess carbon? 2Fe2O3 + 3C ? 4Fe + 3CO2

Transcript

00:01 This question has multiple parts, so it's a little longer.

00:03 So question for part a.

00:06 We are looking at this equation here.

00:12 Aluminum sulfate, mixing with water, to give you aluminum hydroxide plus hydrogen sulfide.

00:26 And to balance that, i already, i have two aluminum on this side.

00:30 I only have one on this side.

00:32 So if i put a two there, that balances my aluminum.

00:34 I have three sulfur.

00:37 I need to put a three there to make three sulfur.

00:40 On this side, i have six hydrogen and six hydrogen.

00:44 So that's 12 hydrogen in total.

00:48 So between this, i have six hydrogen and six hydrogen for 12, which means i'm going to need a six here to make 12 hydrogen, which gives me six oxygen, and i have six oxygen.

01:01 So it's now balanced.

01:03 So between part a, that was part a.

01:06 So part b and c is basically telling me i am mixing 52 .34 grams of the aluminum sulfate, and i want to know how much water, aluminum hydroxide, and dihydrogen sulfide i have.

01:23 So the first thing i'm going to do is write down the molar mass of each of them.

01:27 So when i find the molar mass of aluminum sulfate, i get 150 .17 grams per mole, 18 .02, grams per mole, 78 .01 grams per mole, and 34 .09 grams per mole.

01:48 Because to find the mass of all these things, i know i'm going to need to use the molar mass.

01:54 So the first thing i'm going to do off to the side is i'm going to convert my mass of aluminum sulfate to moles of aluminum sulfate.

02:04 So i'm going to take that 52 .34 grams of aluminum sulfase, knowing that in one mole of aluminum sulfase, i have 150 .17 grams of aluminum sulfate, which is going to give me 0 .3485 moles of aluminum sulfate.

02:35 So i know i have 0 .3485 moles of aluminum sulfate.

02:43 So part b, i'm going to take that moles of aluminum sulfate, and i'm going to convert that to moles of water.

02:57 And i'm going to do that knowing that there's six, for every six moles of water, i have one mole of aluminum sulfate.

03:03 So for every six moles of water, i have one mole of aluminum sulfate, which means i have 2 .091 moles of water.

03:20 Yes? so i know i have 2 .091 moles.

03:27 I have it in water, sorry, h2o.

03:39 I know that in 18 .02 grams of water, i have one mole of water, which is going to give me 37 .68 grams of water...

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