Test #1 Review. 1.Which pair of atoms represents nuclei that have the same number of neutrons? a. 56 Co and 58 Co b. 57 Mn and 57 Fe c. 58 Ni and 57 Fe.

Slides:

Advertisements

Similar presentations

What is the % composition of carbon in benzene (C6H6)?

Advertisements

Chapter 3 Atomic masses Average atomic mass –Ex. What is the avg. atomic mass of a sample that is 69.09% amu and 30.91% amu? –0.6909(62.93amu)

Stoichiometry A measure of the quantities consumed and produced in chemical reactions.

Chemical Stoichiometry

Chapter 9 Stoichiometry.

AP Chemistry Chap. 3 Stoichiometry, Part Chemical Equations (p. 100)- shows a chemical change. Reactants on the LHS, products on the RHS. Bonds.

Chapter 9 Chemical Quantities Chemistry B2A Formula and Molecule Ionic & covalent compounds  Formulaformula of NaCl Covalent compounds  Molecule molecule.

Chemical Reactions H2H2 + O 2  H2OH2O reacts with to yield reactantsproduct 2 H atoms 2 O atoms 1 O atom conservation of mass (g) (l) balanced.

Percentage yield Perform calculations to determine the percentage yield of a reaction Atom Economy Perform calculations to determine the Atom Economy of.

Classic Butter Cookies 2 1/2 cups all-purpose flour 1 cup butter 1/2 cup white sugar 2 eggs 1/2 teaspoon almond extract Bake at 350ºF for 10 minutes.

The Math of Equations Stoichiometry

Chapter 3 - Stoichiometry It is important to be able to quantify the amount of reagent(s) that will be needed to produce a given amount of product(s).

Template by Bill Arcuri, WCSD Click Once to Begin JEOPARDY! Chemistry Final Review.

Stoichiometry Quantitative nature of chemical formulas and chemical reactions Chapter 3 (Sections )

What quantities are conserved in chemical reactions? grams and atoms.

Chapter 3 Test Review -Two short answer and one word problem for each concept - Test will take while. Start Monday and finish by Wednesday. - Homework.

Reaction Stoichiometry.   Deals with the mass relationships that exist between reactants and product  In this type of chemistry, a quantity is given,

Choose Your Category The MoleAverage Atomic Mass and Molar Mass FormulasPercentage Composition Limiting Reactants Percentage Yield and Error Vocab 100.

CHEMISTRY 161 Chapter 4 The Mole. Macroscopic versus Microscopic Worlds 2 H 2 + O 2 2 H 2 O 1 liter water contains about 3.3 X molecules.

Chapter 3 Stoichiometry. Atomic Mass Carbon-12 is assigned a mass of exactly atomic mass units (amu) Masses of other elements are compared to Carbon-12.

1 Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations.

Afra Khanani Period 6 Honors Chemistry March 31 st.

2 pt 3 pt 4 pt 5pt 1 pt 2 pt 3 pt 4 pt 5 pt 1 pt 2pt 3 pt 4pt 5 pt 1pt 2pt 3 pt 4 pt 5 pt 1 pt 2 pt 3 pt 4pt 5 pt 1pt ConversionsGas Laws Molar Mass Equations.

  Chemical Reactions Misc. Gases and Energy Moles Solutions FJ Chemistry.

Stoichiometry Chapters 7 and 9.

Theoretical, Actual, and Percent Yield Problems Example 1.

Hydrate Lab Cu(SO 4 ). H 2 O ----> Cu(SO 4 ) + H 2 O Use the equation above to help answer the following questions: 1.What is the hydrate salt in this.

Stoichiometry Balancing Equations Molecular and Empirical Formulas Percent Composition Mole Conversions

Mass Relationships in Chemical Reactions Chapter 3 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

The Mole Stoichiometry Limiting Reactant % Yield

Mole Jeopardy Moles and Grams Avagadro!Percent Composition Empirical Formula Molecular Formula

Chapter 10 review.

Moles and Stoichiometry Chapters 11 & 12. Counting Particles Particles are counted in moles Types of representative particles Atoms- smallest unit of.

Counting Atoms Chapter 9. MOLE?? Moles of Particles In one mole of a substance, there are 6 x particles.

Agenda: 4/21 Objective: To determine quantities needed for chemical reactions in research or manufacturing: Stochiometry Review: Set up of Stoichiometry.

$100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300.

Mass-Gas Stoichiometry Using a balanced chemical equation, it is possible to determine the volume of a gas if the mass of a reactant or product Is given.

Relative Formula Mass expressed in grams

The Mole & Stoichiometry!

Mass Relationships in Chemical Reactions Chang, Chapter 3 Bylinkin et al, Chapter 1 & 2.

Solving a Stoichiometry Problem 1.Balance the equation. 2.Convert given to moles. 3.Determine which reactant is limiting. 4.Use moles of limiting reactant.

C HAPTER 3 - S TOICHIOMETRY. 3.1 – A TOMIC M ASSES Carbon-12, the relative standard C-12 is assigned a mass of exactly 12 atomic mass units (amu) Masses.

Chemistry Chapter 12 Review Game. Balancing Chemical Equations Stoich #1 (easy) Stoich #2 (more difficult) % Yield 1 point 1 point 1 point 1 point 1 point.

Afra Khanani Period 6 Honors Chemistry March 31 st.

Stoichiometry Warmup I have 1 mole of CO 2 gas at STP. How many grams of CO 2 do I have? How many Liters of CO 2 do I have? How many molecules of CO 2.

Grudgeball Midterm Review. Question 1:  Complete the following chart: Nuclear Symbol # of protons # of neutrons # of Electrons Mass number Charge 30.

1 Chapter 4 Chemical Equations and Stoichiometry.

Can’t directly measure moles Measure units related to moles: –Mass (molar mass) –Number of particles (6.02 x ) –Liters of gas (22.4 Liters at STP)

Chapter 3 Review.

Mass-Mass Conversions 56.0 g N 2 x g N 2 g NH = 1904 = When nitrogen and hydrogen react, they form ammonia gas, which has the formula.

IC5.2.3 Mole calculations © Oxford University Press Mole calculations.

L3: Chemical Formulas and Word Equations Learning Objectives: 1.Understand what information a chemical formula tells you. 2.Write simple word equations.

 Which of the following is an empirical formula? a. C 2 H 6 O 2 b. C 4 H 8 O 10 c. C 2 H 2 O 2 d. C 2 H 3 O 2.

The Mole Introduction to Chemistry. The Mole Atoms and molecules are too small to count out individually Avogadro’s Number = 6.02 x particles /

Mass Relationships in Chemical Reactions

Stoichiometry II.

Stoichiometry Chapter 3

Mass Relationships in Chemical Reactions

Molar Mass and Molar Volume

DO NOW: Answer #1 and #2 in your Packet

Chapter 12 Review.

Chapter 12 Review.

balanced chemical reaction

Stoichiometry Review.

Aim: How do chemists calculate the mass of one mole of a substance?

Introduction to the Mole and Math Concepts

Chapter 9 Key Terms Mole Molar Mass Avogadro's Number Percent Composition Stoichiometry Limiting Reactant Excess Reactant Actual Yield Theoretical Yield.

Stoichiometry Problems

Presentation transcript:

Test #1 Review

1.Which pair of atoms represents nuclei that have the same number of neutrons? a. 56 Co and 58 Co b. 57 Mn and 57 Fe c. 58 Ni and 57 Fe d. 58 Ni and 57 Co e. 59 Ni and 56 Fe

2. Which of the following was used to discover the electron? a.The gold foil experiement b.Deflection of cathode rays by electric and magnetic fields c.The oil drop experiment d.Electrolysis e.The mass spectrometer

3. Which sample contains the greatest number of nitrogen atoms? a mol N2O4 b.0.40 mol N2 c.40. g NH3 d.80. g N2O4

4. How many sodium atoms are in 3.49 grams of sodium?

5. What is the empirical formula of a substance that is 30.% nitrogen and 70.% oxygen? What is the molecular formula if the molar mass is 92 g/mol?

6. A reaction between mL of 1.20 M barium carbonate and 16.0 grams of sodium hydroxide produces grams barium hydroxide and sodium carbonate. a.What is the limiting reactant? b.How many moles of excess reactant are left over? c.What is the theoretical yield of barium hydroxide? d.What is the percent yield of barium hydroxide?

Magnesium hydroxide neutralizes hydrochloric acid to form magnesium chloride and water. Write a balanced chemical equation. How many liters of 1.22 M magnesium hydroxide are needed to neutralize 1.28 L of 0.56 M hydrochloric acid?