CHEM 1127Q Lecture Notes - Lecture 15: Equivalence Point, Thermite, Stoichiometry

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cerisefish201

13 Mar 2019

School

UConn

Department

Chemistry

Course

CHEM 1127Q

Professor

Niluka Wasalathanthri

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CHEM 1127Q Lecture Notes - Lecture 14: Oxidation State

CHEM 1127Q Lecture Notes - Lecture 15: Equivalence Point, Thermite, Stoichiometry

CHEM 1127Q Lecture Notes - Lecture 16: Gravimetric Analysis, Chemical Energy, Sodium Chloride

Document Summary

Topics covered: 4. 3 reaction stoichiometry, 4. 5 quantitative chemical analysis. The numerical relationship between chemical quantities in a balanced chemical equation is called reaction stoichiometry. We can predict the amounts of products that form in a chemical reaction based on the amounts of reactants. We can predict how much of the reactants are necessary to form a given amount of product. We can predict how much of one reactant is required to completely react with another reactant. In a balanced chemical equation, we have a recipe for how reactants combine to form products. Ex: hydrogen and nitrogen combine to form ammonia. 2 are required to react with 2. 50 mol of. Suppose we have 3 cups flour, 10 eggs, and 4 tsp baking powder. **the flour would be the limiting reagent; it is completely consumed and yields the least about of pancakes**

Related Questions

Why must chemical equations be balanced?

Choose all that apply.

	In a balanced chemical equation, the coefficients in front of each reactant and product allow us to predict whether the given reaction is possible or not.
	In a balanced chemical equation, the coefficients in front of each reactant and product allow us to predict whether the reaction requires a catalyst or not.
	In a balanced chemical equation, the coefficients in front of each reactant and product allow us to predict the amount of product that can form from a given amount of reactant.
	In a balanced chemical equation, the coefficients in front of each reactant and product allow us to predict how much of one reactant is required to react with a given amount of another.
	In a balanced chemical equation, the coefficients in front of each reactant and product allow us to predict how much reactants are required to form a given amount of products.

brownarmadillo516

The following are actual student responses to the question: Why is it necessary to balance chemical equations?

The chemicals will not react until you have added the correct ratios.
The correct products will not form unless the right amounts of reactants have been added.
A certain number of products cannot form without a certain number of reactants.
The balanced equation tells you how much reactant you need, and allows you to predict how much product you will make.
A ratio must be established for the reaction to occur as written.

Justify the best choice, and, for choices you did not pick, explain what is wrong with them.

coralplatypus464

To understand how to use stoichiometry to convert between quantities of reactants and products in chemical equations. Stoichiometry describes the quantitative relationships among the reactants and products of a balanced reaction by directly comparing mole ratios. Stoichiometry can be used to convert mass, number of moles, or number of partides between products and reactants, as shown in the flowchart displayed in the figure. (Figure 1) How many grams of NH3 can be produced from 2.21molofN2 and excess HÂ« Express your answer numerically in grams. How many grams of H2 3re needed to produce 10.14g of NH3 ? Express your answer numerically in grams. How many molecules {not moles) of NHa are produced from 8.42 times 10-1g of Hg? Express your answer numerically as the number of molecules. In the following chemical reaction 2 mol of A will react with 1 mol of B to produce 1 mol of A B without anything left over: But what if you re given 2.8 mol of A and 3.2 mol of B7 The amount of product formed is limited by the reactant that runs out first, called the limiting reactant. To identify the limiting reactant, calculate the amount of product formed from each amount of reactant separately: Notice that less product is formed with the given amount of reactant A. Thus. A is the limiting reactant, and a maximum of 1.4 mol of A2B can be formed from the given amounts. If you had excess chlorine, how many moles of of aluminum chloride could be produced from 11 .Og of aluminum'7 Express your answer to three significant figures and include the appropriate units. Part B If you had excess aluminum, how many moles of aluminum chloride could be produced from 16.0g of chlorine gas, Limiting Reactant Procedure Express your answer to three significant figures and include the appropriate units. Part C Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: What is the maximum mass of aluminum chloride that can be formed when reacting 11.0g of aluminum with 16.3g of chlorine17 Express your answer to three significant figures and include the appropriate units.

CHEM 1127Q Lecture Notes - Lecture 15: Equivalence Point, Thermite, Stoichiometry

CHEM 1127Q Lecture Notes - Lecture 14: Oxidation State

CHEM 1127Q Lecture Notes - Lecture 15: Equivalence Point, Thermite, Stoichiometry

CHEM 1127Q Lecture Notes - Lecture 16: Gravimetric Analysis, Chemical Energy, Sodium Chloride

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