When solid lead(II) sulfide ore burns in oxygen gas, the...

When solid lead(II) sulfide ore burns in oxygen gas, the products are solid lead(II) oxide and sulfur dioxide gas. a. Write the balanced chemical equation for the reaction. b. How many grams of oxygen are required to react with $30.0 \mathrm{~g}$ of lead(II) sulfide? c. How many grams of sulfur dioxide can be produced when $65.0 \mathrm{~g}$ of lead $(\mathrm{II})$ sulfide reacts? d. How many grams of lead(II) sulfide are used to produce $128 \mathrm{~g}$ of lead(II) oxide?

When solid lead(II) sulfide ore burns in oxygen gas, the products are solid lead(II) oxide and sulfur dioxide gas.
a. Write the balanced chemical equation for the reaction.
b. How many grams of oxygen are required to react with $30.0 \mathrm{~g}$ of lead(II) sulfide?
c. How many grams of sulfur dioxide can be produced when $65.0 \mathrm{~g}$ of lead $(\mathrm{II})$ sulfide reacts?
d. How many grams of lead(II) sulfide are used to produce $128 \mathrm{~g}$ of lead(II) oxide?

Key Concepts

Balanced Chemical Equations

This concept involves writing a chemical equation where the number of atoms for each element is the same on both the reactant and product sides, in accordance with the law of conservation of mass. The balanced equation provides the essential mole ratios needed for further stoichiometric computations.

Mole Concept

The mole concept links the microscopic world of atoms and molecules to measurable quantities, allowing chemists to count entities by converting between the number of particles and moles using Avogadro's number.

Stoichiometry

Stoichiometry uses the relationships determined in the balanced chemical equation to relate the quantities of reactants and products. It involves using mole ratios to calculate the amounts (in moles or grams) of a chemical that will participate in or be produced by a reaction.

Molar Mass Calculations

Molar mass is the mass of one mole of a substance, usually expressed in grams per mole. This key concept allows the conversion between the mass of a substance and the number of moles, which is essential in stoichiometric problem solving.

Dimensional Analysis

Dimensional analysis is a systematic approach to convert from one set of units to another using conversion factors. In stoichiometry, it is used to transition from grams to moles and then to other units, ensuring that calculations are consistent and accurate.

Transcript

00:02 Okay, so for this problem, there are actually four parts.

00:05 The first part being we have to give the balanced chemical reaction.

00:10 So for part a, it talks about lead sulfide, so that would be pb and the charge is plus two, and sulfide is minus two, therefore it's just pbs.

00:25 So it says lead sulfide solid plus oxygen, oxygen is o2.

00:38 Because it's a diatomic, yields lead oxide, which pv again is plus two, oxygen is minus two, so they cancel each other out, plus sulfur dioxide, so2.

00:58 So we have to balance this chemical reaction.

01:04 Since we're gonna have to have, right now, we only have three oxygen on our reactant side and we can only have even numbers, or sorry, we have three oxygen on our product side, we only have two on our reactant side.

01:17 So i'm going to make this a two, which means we have to have a two over here, which means we have to have two sulfur.

01:31 And when all of a sudden done, we have two, four, six oxygen.

01:35 Therefore, we need three oh -twos.

01:38 And if we count, we have two lead on a reactant side, two lead on our product side.

01:42 We have two sulfur on a reactant side.

01:44 We have two sulfur in our product side.

01:46 And finally, we have six auction on our reactants side, and two plus four, which is six oxygen on our product side.

01:54 So then part b says to convert 30 .0 grams of pvs to grams of o2.

02:07 So if we're going to convert grams to grams, that's going to be three steps.

02:11 First thing we're going to do is get rid of these grams of pvs by putting one mold pvs in the top.

02:21 We're going to find grams by using the periodic table.

02:27 And when we add the mass of lead and sulfur, we get 239 .0 .26, excuse me.

02:39 So then our next step is our molar ratio.

02:43 So to get rid of our moles of pbs, we have put moles of pbs in the bottom.

02:48 Remember, we're going to oxygen.

02:50 However, we can't go straight to grams of o2.

02:52 So instead we're going to make a moles of o2.

02:54 This is where we have to look at our coefficients.

02:57 Of our balanced chemical reaction.

02:59 So pbs would be two, and oxygen would be three.

03:05 And then finally we have to convert to grams of o2.

03:09 So one mole of o2 is gonna go on the bottom and grams of o2 is gonna go in the top, because that's what we're trying to find.

03:18 Grams of o2 is on the periodic table, 16 times 2, which gives us a mass of 32.

03:25 So when all the math is said and done, you multiply 30 times 3 times 32, and then you multiply 239 .2, 6 times 2.

03:31 And then you divide those numbers, you end up with a mass of 6 .02 grams of 02 for part b.

03:44 Part c is another mass to mass, which means it's going to be three steps.

03:49 We're going to start with 65 grams of pbs.

03:54 So the beginning is going to look very similar.

03:56 However, we're getting to grams of s .o2 this time.

04:01 So the first step, again, we have to get rid of our grams of pbs.

04:06 And the only thing that can go with grams is one mole of that substance...

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