Consider the unbalanced chemical equation HCl+Zn →H2+ZnCl2 (a) Balance the equation. (b) Transla

Consider the unbalanced chemical equation HCl+Zn →H2+ZnCl2...

Consider the unbalanced chemical equation $\mathrm{HCl}+\mathrm{Zn} \rightarrow \mathrm{H}_{2}+\mathrm{ZnCl}_{2}$ (a) Balance the equation. (b) Translate the equation into words using the word mole(s) wherever you can. (c) To produce 1 mole of $\mathrm{H}_{2}$ from the reaction you just wrote, how many grams of $\mathrm{HCl}$ and Zn must you combine? (d) What is the theoretical yield in grams of $\mathrm{H}_{2}$ ? (e) You recover $2.00 \mathrm{~g}$ of $\mathrm{H}_{2}$ after carrying out the reaction. What is the percent yield?

Consider the unbalanced chemical equation $\mathrm{HCl}+\mathrm{Zn} \rightarrow \mathrm{H}_{2}+\mathrm{ZnCl}_{2}$
(a) Balance the equation.
(b) Translate the equation into words using the word mole(s) wherever you can.
(c) To produce 1 mole of $\mathrm{H}_{2}$ from the reaction you just wrote, how many grams of $\mathrm{HCl}$ and Zn must you combine?
(d) What is the theoretical yield in grams of $\mathrm{H}_{2}$ ?
(e) You recover $2.00 \mathrm{~g}$ of $\mathrm{H}_{2}$ after carrying out the reaction. What is the percent yield?

Key Concepts

Theoretical Yield

The theoretical yield is the amount of product that is expected to be produced from a chemical reaction when quantities of reactants are completely consumed as predicted by stoichiometry. It serves as an ideal benchmark for evaluating reaction efficiency.

Molar Mass

Molar mass is the mass of one mole of a given substance, normally expressed in grams per mole. It plays an important role in stoichiometric calculations by providing the means to convert between the mass of a substance and the number of moles.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, defined as the ratio of the actual yield (the quantity of product actually obtained) to the theoretical yield, multiplied by 100. It indicates the degree to which a reaction follows its predicted stoichiometry.

Mole Concept

The mole concept is a fundamental principle in chemistry that introduces the mole as a unit to measure the amount of substance. It links the atomic scale with the macroscopic observable amounts through Avogadro's number, which specifies the number of particles in one mole.

Balancing Chemical Equations

This concept refers to the process of ensuring that the number of atoms of each element is the same on both sides of a chemical equation. It is essential because the law of conservation of mass requires that matter is neither created nor destroyed during chemical reactions.

Stoichiometry

Stoichiometry involves using the quantitative relationships among reactants and products in a chemical reaction as represented by a balanced chemical equation. It allows chemists to calculate the amounts of substances consumed and produced, often converting between mass and moles.

Transcript

00:01 All right, here we have another one that's kind of a multi -part question.

00:05 The first thing it wants us to do is balance the equation.

00:09 So we're going to start part a.

00:12 The unbalanced equation is hcl plus zinc yields hydrogen gas and zinc chloride.

00:28 Okay, just by looking at this right off the bat, we have two hydrogens and two chlorines over here on the right.

00:34 And only one of each over here on the left.

00:38 So if we do that, but the two is their co -vision.

00:41 Now i've got two hydrogens, two chlorines, one zinc, and two hydrogens, two chlorines, and one zinc.

00:49 So balancing this one's real simple.

00:51 You just got to add a two in front of the hcl, and you're good to go.

00:55 Okay, to translate that in the words, you could say something like two moles of hydrochloric acid or hcl, plus one mole of zinc will yield one mole of hydrogen.

01:05 Gas and one mole of zinc chloride.

01:12 Question c there, to produce one mole of h2 from the reaction you just wrote, how many grams of hcl and zinc must be combined.

01:22 So if we're making one mole of h2, like it says right here, there's no coefficient, wants to know how many grams of each of these we would need.

01:29 Okay.

01:30 To do that, we're going to need a periodic cable because we need to know the atomic weights of these elements.

01:43 So we need to find the molar mass of each of them, and then multiply by however many moles of that compound we're going to be using.

01:49 So for the hydrochloric acid, it's pretty simple.

01:52 Hydrogen, if we look on the periodic table, has a mass of 1, and chlorine has a mass of 35, 34 .5, something like that.

02:08 35 .5...

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