When solid lead(II) sulfide reacts with oxygen gas, the...

When solid lead(II) sulfide reacts with oxygen gas, the products are solid lead(II) oxide and sulfur dioxide gas. a. Write the balanced equation for the reaction. b. How many grams of oxygen are required to react with $29.9 \mathrm{~g}$ of lead(II) sulfide? c. How many grams of sulfur dioxide can be produced when $65.0 \mathrm{~g}$ of lead(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 reacts with oxygen gas, the products are solid lead(II) oxide and sulfur dioxide gas.
a. Write the balanced equation for the reaction.
b. How many grams of oxygen are required to react with $29.9 \mathrm{~g}$ of lead(II) sulfide?
c. How many grams of sulfur dioxide can be produced when $65.0 \mathrm{~g}$ of lead(II) sulfide reacts?
d. How many grams of lead(II) sulfide are used to produce $128 \mathrm{~g}$ of lead(II) oxide?

Key Concepts

Stoichiometry

Stoichiometry is the aspect of chemistry that involves calculating the quantitative relationships between reactants and products in a chemical reaction. It utilizes the balanced chemical equation and the mole concept to determine how much of each reactant is needed or how much product can be formed.

Mass-Mole Conversions

Mass-to-mole and mole-to-mass conversions are critical procedures in stoichiometry, allowing one to translate between the mass of a substance and the number of moles using its molar mass. These conversions form the basis for determining the stoichiometric relationships in a reaction.

Balancing Chemical Equations

Balancing chemical equations ensures that the number of atoms of each element is the same on both sides of a reaction, adhering to the law of conservation of mass. This process is essential for determining the correct stoichiometric coefficients, which are used in subsequent quantitative calculations.

Mole Concept and Molar Mass

The mole is a fundamental unit in chemistry representing a specific number of particles, typically 6.022 x 10^23. Molar mass, the mass of one mole of a substance, is key for converting between the mass of a substance and the number of moles. This conversion is crucial for any quantitative analysis in chemical reactions.

Transcript

00:02 That occurs when solid lead 2 sulfide reacts with oxygen gas.

00:07 The products of this reaction are solid lead 2 oxide and sulfur dioxide gas.

00:13 Our first order of business, question a, is to write the balanced chemical equation.

00:30 And that's pretty easy.

00:31 We've got pbs, solid, lead 2 sulfide, reacting with oxygen gas, and our products will be lead 2 oxide and sulfur dioxide gas.

00:53 Okay, taking a look here.

00:55 I'm gonna have to have probably a 2 in front of this, which give me a 2 here and a 2 here or and a 3 here.

01:09 So 2, 3, 2, 2.

01:11 That looks good to me.

01:12 There's my first answer.

01:15 Let me go get a highlighter and highlight that for you.

01:23 There's part a.

01:29 For part b.

01:32 Let me get back to my question.

01:34 Lost my question here.

01:40 Where is my question? how many grams of oxygen to react with 29 .9 grams of the lead 2 sulfide.

02:10 Okay, that one will be pretty easy.

02:14 I just got to get to a molar mass tab here.

02:21 29 .9.

02:27 29 .9 grams of lead 2 sulfide.

02:34 Okay, my molar mass for lead 2 sulfide, and i just look these up in a molar mass tab.

02:40 Pretty simple.

02:48 Let me go find it.

02:51 Where's my molar mass tab? pbs.

02:57 And that will be 239 .27.

03:10 And then what we use for oxygen, 3 moles of oxygen for my balanced chemical equation and 2 moles of my lead 2 sulfide.

03:21 Finally, we'll multiply that by 32 .00 grams of oxygen per mole of oxygen, which is the molar mass of oxygen.

03:31 29 .9 times 3 times 32 divided by 239 .27 divided by 2.

03:41 And i get 5 .998 is 6 .0.

04:02 I'm gonna go look at something quick...

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