DOCX

Review from Unit 6- please perform the following conversions on

By Richard Lee,2014-04-12 22:00
8 views 0
Review from Unit 6- please perform the following conversions on

Unit 11 Worksheets: Chapter 12 Stoichiometry Page | 1

    Name: Block

    Review from Unit 9- please perform the following conversions on your own paper. Show all work.

    Include correct units. Enclose your answers in a box.

    Remember: 23Avogadro’s number is: 6.022 x 10 particles = 1 mole

    Molar Volume only applies to gases at STP and is: 22.4 L = 1 mol

    Molar Mass can be found on the periodic table and is: value from PT g = 1 mol

    (the formula must be the same on both sides of all of these conversions)

    1. Convert from 5 L of nitrogen gas to moles of nitrogen gas.

    2. Convert from 5 moles of oxygen gas to molecules of oxygen gas.

    3. Convert from 5 L of nitrogen gas to atoms of nitrogen.

    4. Convert from 5 moles of oxygen gas to atoms of oxygen.

    5. Convert from 6 moles of water to grams of water.

    6. Convert from 6 moles of water to grams of hydrogen. 237. Convert from 5.43 x 10 formula units of NaCl to moles of NaCl.

    Unit 11 Worksheet 1: Section 12.1 Interpreting equations. (there are 3 questions)

    See Page 357 in the book for help.

    1. Fill out the chart. Interpret the reaction in terms of each of the categories indicated in the left column:

    Reaction: H+ O ; HO 2 222

    Atoms of each

    element:

    Molecules of each

    substance:

    Moles of each

    substance:

    Grams of each

    substance:

    Volume of each

    substance assuming

    STP:

    Reaction: 2C + O; 2CO 2

    Atoms of each

    element:

    Molecules of each

    substance:

    Moles of each

    substance:

    Grams of each

    substance:

    Volume of each

    substance assuming

    STP:

    2. Balance this equation: CHOH (l) + O (g) ; CO (g) + HO (g) 25222

     a. Interpret the equation in terms of number of molecules.

     b. Interpret the equation in terms of number of moles.

Unit 11 Worksheets: Chapter 12 Stoichiometry Page | 2

    Name: Block

    c. Show that the balanced equation obeys the law of conservation of mass. (hint- show that the mass is

    the same on both sides of the equation)

3. Explain why this statement is true: “Mass and atoms are conserved in every chemical reaction, but moles will

    not necessarily be conserved.”

Unit 11 WORKSHEET 2: Section 12.2 Chemical Calculations

    SHOW ALL WORK, INCLUDE CORRECT UNITS, and ENCLOSE YOUR ANSWER IN A BOX USE

    YOUR OWN PAPER PLEASE!

     For each problem you should consider:

    1) How will you convert from the units given to moles?

    a. Remember to consider Avogadro’s number, molar mass, and molar volume

    2) What mole ratio will you use?

    3) How will you convert from moles to the desired units?

    a. Remember to consider Avogadro’s number, molar mass, and molar volume.

    1. This equation shows the formation of aluminum oxide:

     4Al(s) + 3O(g) ; 2AlO(s) 223

    a. How many moles of aluminum are needed to form 8.4 moles of aluminum oxide?

    b. How many moles of oxygen are needed to form 8.4 moles of aluminum oxide?

    c. How many moles of oxygen are needed to completely react with 17.6 moles of aluminum?

    d. How many moles of aluminum oxide are formed when 0.65 moles of oxygen reacts with

    aluminum?

    2. Acetylene gas is produced by adding water to calcium carbide in this reaction:

    CaC(s) + 2HO (l) ; CH(g) + Ca(OH) (aq) 22222

    a. How many grams of acetylene are produced by adding water to 4.00 grams of calcium carbide?

    (calcium carbide is CaC. Acetylene is CH) 222

    b. How many moles of calcium carbide are needed to react completely with 23 grams of water?

    3. 2KClO(s) ; 2KCl (s) + 3O(g) 32

    a. How many molecules of oxygen are produced by the decomposition of 7.23 grams of potassium

    chlorate? 25 b. How many formula units of KCl are produced by the decomposition of 7.65 x 10formula units

    of KClO? 354c. How many grams of oxygen are produced by the decomposition of 8.98 x 10 formula units of

    potassium chlorate?

    4. The equation for the combustion of carbon monoxide is:

    2CO(g) + O(g) ; 2 CO (g) 22

    a. How many liters of oxygen are required to burn 5.45 L of carbon monoxide?

    b. How many liters of carbon dioxide are produced from 7.34 L of oxygen provided you have

    unlimited CO?

    c. How many liters of CO are required to react completely with 32 grams of O? 2

    5. How many grams of silver chloride are produced from 5.0 grams of silver nitrate reacting with an excess

    of barium chloride? (hint: balance your equation first. Excess just means you can ignore that reactant)

    __AgNO + BaCl ; __AgCl + Ba(NO) 3232

Unit 11 Worksheet 3- Limiting reagents Section 12.3

Unit 11 Worksheets: Chapter 12 Stoichiometry Page | 3

    Name: Block

    SHOW YOUR WORK, INCLUDE CORRECT UNITS, and ENCLOSE YOUR ANSWERS IN A BOX. Limiting Reagent and Excess Reagent

    1. What is the limiting reagent in each of the following situations if you wish to make a table with 4 legs

    and a top.

    a. You have 8 legs and 3 tops.

    b. You have 10 legs and 4 tops.

    c. You have 12 legs and 2 tops.

    d. You have 16 legs and 7 tops.

    2. The equation for the complete combustion of ethene is CH (g) + 3 O ; 2CO + 2 HO. If 5.6 moles 24222

    of CH is reacted with 8.70 moles of oxygen, 24

    a. Identify the limiting reagent

    b. Calculate the moles of water produced

    c. Identify the excess reagent

    3. The equation for the combustion of magnesium is 2Mg + O ; 2MgO 2

    a. If you have 10.0 moles of Mg and 4.0 moles of oxygen, what is the limiting reagent?

    b. How many moles of magnesium oxide are produced?

    4. Hydrochloric acid reacts with zinc to produce hydrogen gas. 2HCl + Zn ; ZnCl + H 22

    a. Identify the limiting reagent if you have 7.00 g of HCl and 9.00 g of Zn.

    b. How many grams of hydrogen can be produced in this situation?

    5. Copper (II) sulfate reacts with zinc to create copper and zinc sulfate.

    a. Identify the limiting reagent if 10.00 g of Copper (II) sulfate react with 40.0 g of zinc. (HINT:

    Write the correct balanced equation first!!!)

    b. How many grams of copper can be produced in this situation?

    6. Silver nitrate reacts with sodium chloride to form sodium nitrate and silver chloride.

    a. How many grams of silver chloride can be produced from 7.00 g of sodium chloride and 8.00 g

    of silver nitrate?

    Percent Yield

    7. When 90.8 g of iron (III) oxide reacts with an excess of carbon monoxide, 40.0 grams of iron is

    produced. FeO + 3CO ; 2Fe + 3 CO. What is the percent yield of this reaction? 232

    8. When 90.0 g of silicon dioxide is heated with an excess of carbon, 41.0 g of silicon carbide is produced.

    SiO + 3C ; SiC + 2CO. What is the percent yield of this reaction? 2

    9. If 75.0 g of iron (II) carbonate is heated with an excess of oxygen, 45.0 g of iron (III) oxide is produced.

    The other product is carbon dioxide.

    a. What is the percent yield of this reaction? (HINT: Write a balanced equation first!!!!)

    10. When 50.0 g of silicon dioxide is heated with an excess of carbon, 32.2 grams of silicon carbide is

    produced. SiO(s) + 3C(s) ; SiC (s) +2CO(g) 2

    a. What is the percent yield of this reaction?

    b. How many grams of CO gas are made?

    11. If the reaction below proceeds with a 96.8% yield, how many grams of CaSO are formed when 5,240 4

    grams of SO react with an excess of CaCO and O? 2CaCO(s) + 2SO(g) + O(g) ; 2CaSO(s) 2323224

    +2CO(g) 2

For more practice: http://www2.hmc.edu/%7Ekarukstis/chem21f2001/tutorials/problemsStoichiFrame.html

    http://www.chemistrycoach.com/tutorials-2.html

Chapter 11 Study Guide

Unit 11 Worksheets: Chapter 12 Stoichiometry Page | 4

    Name: Block

    Remember to look over the goals in your notes, read your book, read your notes, look at old worksheets. If you need more practice problems, you can get them from my website or come see me for a copy. The more you practice, the better you will do on the test.

    To receive credit for questions 4-14: Show all work, include correct units, and enclose your answers in a

    box. Please show work in the dimensional analysis format, just as we’ve done in class.

    1. What is always conserved in any chemical reaction? (You may select more than one answer: moles, mass, atoms, molecules, liters)

    2. Which of the following statements is true about this reaction: N (g) + 3H (g) ; 2NH (g) 223

     a. 8 atoms of reactants rearrange to form 5 atoms of products

     b. 22.4 L of reactants form 22.4 L of products

     c. 4 grams of reactants form 2 g of products

     d. 4 L of reactants form 2 L of products

     e. 4 moles of reactants form 2 moles of products

    3. What makes actual yield different from theoretical yield? (answer in full sentences please) 4. If a total of 9 mol of NaHCO and 6 mol of CHO react, how many moles of NaCHO will be produced?

    3NaHCO(aq) + CHO(aq) 3CO(g) + 3HO(s) +NaCHO(aq)

    5. How many grams of CO are needed to react with an excess of FeO to produce 8.5 g Fe?

    FeO(s) + 3CO(g) 3CO(g) + 2Fe(s)

    6. How many liters of O are needed to react completely with 89 L of HS at STP?

    2HS(g) + 3O(g) 2SO(g) + 2HO(g)

    7. For the reaction 2Na(s) + Cl(g) 2NaCl(s), how many grams of NaCl could be produced from 5.5 g of Na and 2.0 L of Cl (at STP)?

    8. Solid sodium reacts violently with water, producing heat, hydrogen gas, and sodium hydroxide. How many molecules of hydrogen gas are formed when 54g of sodium are added to water?

    2Na + 2HO 2NaOH + H

    9.Consider the following reaction:

    2HS(g) + 3O(g) 2SO(g) + 2HO(g)

    If you have 4 mol of HS reacting with excess oxygen, and the actual yield is 64.08g of water, what is the percent

    yield of the reaction?

    10. What is the limiting reagent when 224 g of nitrogen react with 60.6 g of hydrogen?

    N(g) + 3H(g) 2NH(g)

    11. This equation shows the formation of aluminum oxide: 4Al(s) + 3O(g) ; 2AlO(s) How many moles of 223

     aluminum are needed to form 7.8 moles of aluminum oxide? 25 12. How many formula units of KCl are produced by the decomposition of 4.5 x 10formula units of KClO? 3

     2KClO(s) ; 2KCl (s) + 3O(g) 32

    13. The equation for the combustion of carbon monoxide is:

    2CO(g) + O(g) ; 2 CO (g) 22

     How many liters of CO are required to react completely with 54 grams of O? 2

    14. How many formula units of AgNO are needed to react completely with 5.74 moles of Cu? The equation is: 3

     2 AgNO + Cu ; Cu(NO) + 2 Al 332

    BONUS

    15. If 45.5 g of H are reacted with excess CO, how many grams of CHOH are produced, based on a yield of 98%? CO(g) + 2H(g) CHOH(l)

Report this document

For any questions or suggestions please email
cust-service@docsford.com