Chemistry Chapter 11 Study Guide
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Chemistry Chapter 11 Study Guide

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Questions and Answers

What determines how much product can actually form in a chemical reaction?

The amount of reactant present at the start of a chemical reaction.

When do chemical reactions stop?

When one of the reactants is used up.

What is stoichiometry?

The study of quantitative relationships between the amounts of reactants used and amounts of products formed by a chemical reaction.

What is stoichiometry based on?

<p>The Law of Conservation of Mass.</p> Signup and view all the answers

What is a mole ratio?

<p>A ratio between the number of moles of any two substances in a balanced equation.</p> Signup and view all the answers

What is a mole ratio for the equation: 2Al(s) + 3Br₂(l) → 2AlBr₃(s)?

<p>2 mol Al : 3 mol Br₂.</p> Signup and view all the answers

How many mole ratios can be written for the equation: 4H₂(g) + O₂(g) → 2H₂O(l)?

<ol start="6"> <li></li> </ol> Signup and view all the answers

What does every stoichiometric problem require?

<p>A balanced chemical equation.</p> Signup and view all the answers

What do all stoichiometric problems begin with?

<p>A balanced chemical equation.</p> Signup and view all the answers

What does the endpoint of a stoichiometric calculation depend on?

<p>The desired unit of the unknown substance.</p> Signup and view all the answers

When does a chemical reaction stop?

<p>When one of the reactants is used up.</p> Signup and view all the answers

Reactions proceed until?

<p>One of the reactants is used up and the other is left in excess.</p> Signup and view all the answers

The limiting reactant limits the ______ of the reaction, and thereby determines the _____________-.

<p>extent, amount of product formed.</p> Signup and view all the answers

What are excess reactants?

<p>All the leftover, unused reactants.</p> Signup and view all the answers

Sometimes there's ___ leftover.

<p>no.</p> Signup and view all the answers

Why is determining the limiting reactant important?

<p>The amount of product formed depends on the reactant.</p> Signup and view all the answers

Using an excess reactant can ________ the reaction.

<p>Speed up.</p> Signup and view all the answers

Using an excess reactant can _______________ to ________.

<p>drive a reaction, completion.</p> Signup and view all the answers

Percent yield is a measure of the _________ of a reaction.

<p>efficiency.</p> Signup and view all the answers

Laboratory reactions do not always produce?

<p>the calculated amounts of products.</p> Signup and view all the answers

Reactants stick to _________. There can be ________ reactants. __________ reactions form other products.

<p>containers, impure, competing.</p> Signup and view all the answers

What is the theoretical yield?

<p>The maximum amount of a product that can be formed from a given amount of reactant.</p> Signup and view all the answers

What is the actual yield?

<p>The amount of product actually produced when the chemical reaction is carried out in an experiment.</p> Signup and view all the answers

What is the percent yield of a product?

<p>The ratio of the actual yield expressed as a percent.</p> Signup and view all the answers

Why is percent yield important?

<p>The cost effectiveness of many industrial manufacturing processes.</p> Signup and view all the answers

Study Notes

Chemical Reaction Fundamentals

  • The initial amount of reactant influences the maximum possible product yield in a reaction.
  • A reaction ceases when one reactant is completely consumed.

Stoichiometry Overview

  • Stoichiometry examines the quantitative relationships between reactants and products in chemical reactions.
  • Fundamental principle based on the Law of Conservation of Mass, which states that mass is neither created nor destroyed in a chemical reaction.

Mole Ratios

  • A mole ratio quantifies the relationship between the number of moles of two substances in a balanced equation.
  • Example ratio from the equation 2Al(s) + 3Br₂(l) → 2AlBr₃(s): 2 mol Al : 3 mol Br₂.
  • Six different mole ratios can be derived from the equation 4H₂(g) + O₂(g) → 2H₂O(l).

Stoichiometric Calculations

  • Every stoichiometric problem starts with a balanced chemical equation.
  • The concluding phase of a calculation depends on the desired unit of the unknown substance.

Limiting and Excess Reactants

  • A reaction concludes when one reactant is exhausted, leaving others in excess.
  • The limiting reactant determines the extent of the reaction and the quantity of product produced.
  • Excess reactants enhance reaction efficiency and can drive reactions to completion.

Yield Concepts

  • Percent yield assesses a reaction's efficiency, calculated as (actual yield/theoretical yield) x 100%.
  • The theoretical yield is the predicted maximum quantity of product from specific reactant amounts.
  • Actual yield represents the real amount of product obtained in laboratory experiments.

Practical Considerations in Reactions

  • Laboratory reactions may yield less product than anticipated due to reactants adhering to containers, impure reactants, or competing reactions.
  • Understanding percent yield is crucial for evaluating the economic effectiveness of industrial manufacturing processes.

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Description

This quiz explores essential concepts from Chemistry Chapter 11, focusing on reactants, products, and stoichiometry. Test your understanding of the relationships and quantities in chemical reactions with these flashcards. Ideal for students preparing for exams or reviews.

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