Silver nitrate, AgNO, reacts with sodium chloride, NaCl, in aqueous solution to form solid silve

Silver nitrate, AgNO, reacts with sodium chloride, NaCl, in...

Silver nitrate, AgNO, reacts with sodium chloride, $\mathrm{NaCl},$ in aqueous solution to form solid silver chloride, AgCl(s), and aqueous sodium nitrate, $\mathrm{NaNO}_{3}(a q) .$ Suppose you start with 6.3 $\mathrm{g}$ of AgNO $_{3}$ and 4.5 $\mathrm{g}$ of $\mathrm{NaCl}$ . a. Write a balanced chemical equation for this reaction. b. How many moles of each reactant are you starting with? c. What is the limiting reactant? d. How many grams of each product do you expect to produce? e. How many grams of excess reactant do you expect to have when the reaction is complete?

Silver nitrate, AgNO, reacts with sodium chloride, $\mathrm{NaCl},$ in aqueous solution to form solid silver chloride, AgCl(s), and aqueous sodium nitrate, $\mathrm{NaNO}_{3}(a q) .$ Suppose you start with 6.3 $\mathrm{g}$ of AgNO $_{3}$ and 4.5 $\mathrm{g}$ of $\mathrm{NaCl}$ .
a. Write a balanced chemical equation for this reaction.
b. How many moles of each reactant are you starting with?
c. What is the limiting reactant?
d. How many grams of each product do you expect to produce?
e. How many grams of excess reactant do you expect to have when the reaction is complete?

Key Concepts

Stoichiometry

Stoichiometry involves the quantitative relationships among reactants and products in a chemical reaction based on the balanced chemical equation. This concept allows for the calculation of amounts of reactants needed and products produced, using mole ratios derived from the equation.

Theoretical Yield and Excess Reactant Calculation

The theoretical yield is the maximum amount of product that can be formed from the given quantities of reactants, as predicted by stoichiometric calculations. Calculating the excess reactant involves determining the amount of the reactant remaining after the reaction has gone to completion, by subtracting the quantity consumed based on the limiting reactant's stoichiometry.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first during a chemical reaction, thereby preventing further reaction from occurring. Identifying the limiting reactant is crucial because it determines the maximum amount of product that can be formed.

Balanced Chemical Equation

A balanced chemical equation represents the chemical reaction with the same number of atoms for each element on both the reactant and product sides. This is essential for ensuring mass conservation and establishing the stoichiometric coefficients that are used in subsequent calculations.

Mole Concept

The mole is a fundamental unit in chemistry that connects the mass of a substance to the number of particles it contains using its molar mass. Converting grams to moles (and vice versa) is a critical skill for quantifying reactants and products in a chemical reaction.

Transcript

00:02 Question number five is a multi -step question regarding limiting reactants.

00:10 However, it's set up in such a fashion where each previous part prepares you for, in part, the next part.

00:21 The reaction, which they ask you to write first in part a, is sodium chloride reacting with silver nitrate, producing silver chloride solid and sodium nitrate.

00:34 It is balanced as written, no coefficients are required.

00:39 In part b, it asks you to determine how many moles of each reactant are you starting with.

00:44 Well, they tell us we're starting with 6 .3 grams of silver nitrate.

00:50 So all we need to do is divide that by the molar mass of silver nitrate in order to get the moles silver nitrate, 3 .71 times 10 to the negative 2.

01:01 We are also starting with 4 .5 grams.

01:05 Sodium chloride.

01:08 We can get moles sodium chloride by dividing by molar mass sodium chloride which is 7 .70 times 10 to the negative 2.

01:17 Part c asks you to determine what is the limiting reactant.

01:22 To do this appropriately you need to figure out how many moles of either product just choose one can be created with these many moles of reactant.

01:35 So we'll convert the 3 .71 times 10 to the negative 2 mole's silver nitrate into moles silver chloride, this being the product i've chosen, and we get 3 .71 times 10 to the negative 2 moles silver chloride can be made from the amount of silver nitrate we have.

01:54 Then we'll take the 7 .70 times 10 to negative 2 moles sodium chloride, and the stoichiometry here is also 1 to 1.

02:03 It's one to one for everything throughout.

02:07 And we get 7 .70 times 10 to negative 2 moles silver chloride...

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