Honors Chemistry Unit 7 Review

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Questions and Answers

Which of the following has the greatest number of atoms? a. 26.98 g of Al b. 1 mole of S c. 5 moles of O2 d. 18.02 g H2O e. All are the same

26.98 g of Al

5 moles of O2 (correct)

1 mole of S

18.02 g H2O

All are the same

Calculate the molar mass of manganese (IV) oxalate.

206.11 g/mol

How many moles are in 53.0 g of CH4?

3.30 moles

What is the mass of 6.9x10^25 molecules of NO?

1,227.48 g Signup and view all the answers

Which of the following iron compounds contains the greatest percentage of iron: pyrite (FeS2), hematite (Fe2O3), or siderite (FeCO3)?

Hematite (Fe2O3) Signup and view all the answers

Determine the percent composition of Ca(NO3)2.

20.04% Ca, 61.25% N, 18.71% O Signup and view all the answers

A fluoride of aluminum is 67.87% F. What is the formula of this compound?

AlF3 Signup and view all the answers

The empirical formula of C2H5OH is __________.

CH3 Signup and view all the answers

The empirical formula of C6H12O6 is __________.

CH2O Signup and view all the answers

What is the empirical formula for a compound that is 40.00% C, 6.713% H and 53.28% O by mass?

C3H6O Signup and view all the answers

If the molecular mass of a compound is 60.052 g, what is its molecular formula if the empirical formula is C3H6O?

C6H12O2 Signup and view all the answers

What is the limiting reactant if 14.0 g N2 is mixed with 9.0 g H2?

H2 Signup and view all the answers

How much excess reactant is left over after the reaction?

0 g Signup and view all the answers

What is the theoretical yield of NH3?

16.8 g Signup and view all the answers

What is the percent yield if 16.1 g of NH3 actually forms?

96.9% Signup and view all the answers

What is collision theory?

A theory stating that for a reaction to occur, reactants must collide with sufficient energy and proper orientation. Signup and view all the answers

What are the requirements for a successful collision?

Sufficient energy and proper orientation. Signup and view all the answers

How would increasing the temperature affect the rate of a reaction?

Increase Signup and view all the answers

At equilibrium, the amount of products must equal the amount of reactants.

False Signup and view all the answers

During equilibrium, the concentration of the products does not change.

True Signup and view all the answers

A collision between reactants is all that is needed to cause a reaction.

False Signup and view all the answers

If K > 1, __________ are favored.

products Signup and view all the answers

If K < 1, ______________ are favored.

reactants Signup and view all the answers

What are the definitions for acids & bases?

Acid: A substance that donates protons; Base: A substance that accepts protons. Signup and view all the answers

What is meant by the term amphiprotic?

A substance that can both donate and accept protons. Signup and view all the answers

What is specific heat capacity?

The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius. Signup and view all the answers

Calculate the pH of a solution with [H+] = 0.00100 M.

3.00 Signup and view all the answers

What is an indicator and what is it used for?

An indicator is a substance that changes color at a particular pH level, used to determine acidity or alkalinity. Signup and view all the answers

Study Notes

Unit 7 – The Mole

Understand the mole concept for estimating quantities in reactions.
Calculate molar mass from chemical formulas and names.
Convert between particles, mass, and volume in chemical calculations.
Determine percent composition for compounds based on element mass.
Identify empirical and molecular formulas from composition data.

Unit 8 – Balancing Equations and Stoichiometry

Recognize types of chemical reactions.
Balance chemical equations using stoichiometric coefficients.
Derive chemical equations from word problems.
Use balanced equations for reactant/product ratios.
Convert between grams, particles, and liters during reactions.
Identify the limiting reactant and calculate excess reactant and theoretical yield.
Determine percent yield based on actual and theoretical yield.

Unit 9 – Reactions and Solutions

Differentiate between saturated, unsaturated, and supersaturated solutions.
Explain solubility concepts at both macroscopic and particle levels.
Use solubility rules to assess the solubility of ionic compounds.
Write solvation equations showing the dissociation of soluble ionic compounds.
Construct and interpret molecular, complete ionic, and net ionic equations.
Solve concentration problems using molarity and dilution equations.

Unit 10 – Equilibrium

Identify factors affecting reaction rates.
Explain how equilibrium is achieved in reversible reactions.
Write equilibrium constant expressions and calculate K values from reactions.
Analyze reaction extent through K value magnitudes.
Apply ICE tables for calculating equilibrium concentrations.
Utilize LeChatelier’s principle for predicting shifts in equilibrium.

Unit 11 – Acids and Bases

Define acids and bases using Arrhenius and Bronsted-Lowry theories.
Identify conjugate acid-base pairs in reactions.
Recognize key physical and chemical properties of acids and bases.
Calculate H⁺ and OH⁻ concentrations using Kw relationships.
Describe and compute pH values for acidic and basic solutions.
Explain acid-base reactions, including titrations and stoichiometric calculations.

Unit 12 – Thermochemistry

Distinguish between exothermic and endothermic reactions based on enthalpy.
Draw energy diagrams highlighting ΔH and activation energy.
Understand the impact of specific heat capacity on thermal properties.
Perform calculations with the specific heat formula.
Use calorimetry to determine energy changes in reactions and apply Hess’s Law for ΔH calculations.

Important Concepts and Example Calculations

Molar mass of compounds, percentage composition calculations.
Limiting reactant identification in stoichiometric equations.
Equilibrium constant calculations and Q comparisons to predict shifts.
Capitalize on the relationship between pH, [H⁺], and [OH⁻] in aqueous solutions.
Use reaction enthalpy to calculate energy changes in chemical processes.

Noteworthy Questions

Key problem-solving questions regarding mole conversions, balancing equations, and equilibrium states.
Practical applications of acid-base neutralization, as well as calorimetry for energy calculations.
Significant equations for solubility predictions, including molecular forms and precipitation reactions.

Tips for Exam Preparation

Practice calculations involving molar mass and concentration.
Engage in problems that require balancing equations and deriving net ionic equations.
Familiarize with equilibrium concepts and the significance of K and Q values.
Utilize sample acidic and basic titration problems for proficiency in pH calculations.

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Description

Prepare for the second semester exam in Honors Chemistry with this quiz focused on Unit 7: The Mole. Test your understanding of mole concepts, molar mass calculations, and conversions between particles, mass, and volume. Make sure you can also determine percent composition from formulas.