Predicting Products Lab Name

Predicting Products Lab Name

Predicting Products LabName:

Chemistry 5.0 - EquationsDate: Period:

Purpose: The Purpose of this lab is to perform a series of ______, make careful ______,

identify ______, and write ______to describe the reactions.

Pre-lab Questions:

1. What constitutes a positive test for each of the following gases?

  1. oxygen (O2): ______
  2. hydrogen (H2):______
  3. water vapor (H2O):______
  4. ammonia (NH3):______
  5. carbon dioxide (CO2)______and/or ______

2. What is the proper way to smell a substance in the lab? ______

3. What is the role of a catalyst in a reaction? How can you tell if when a substance serves as a catalyst?

______

Materials:goggles/apron2 pieces of magnesium ribboncrucible tongs

Bunsen burnerwatch glass6 test tubes

graduated cylindertest-tube racktest-tube clamp

3 wooden splintscopper turnings well plate

ammonium carbonate3% H2O2spatula

cobalt chloride paper limewater (Ca(OH)2 solution)matches

0.1 M potassium iodide (KI)0.1 Mlead nitrate (Pb(NO3)2

copper carbonate (CuCO3) one-hole rubber stopper glass tube elbow

manganese dioxide (MnO2)2.0 M Hydrochloric acid (HCl)

Procedure:

Read the procedure for each reaction in its entirety before doing it so that you have the necessary materials to complete the procedure. Wear goggles and an apron throughout the entire lab. Be sure to tie back long hair. Write detailed observations in the Chart on page 3. Follow disposal instructions.

Reaction 1:Obtain a jar of Cu powder and a crucible from the lab bench and weigh the empty, clean crucible. Add about 1.00 g of Cu powder and determine the actual mass of copper to the nearest .001 g and record. Place the crucible on a clay triangle and heat it strongly in a Bunsen burner flame for 5 minutes. Allow the crucible to cool and weigh it again. Record the initial and final appearances of the copper as well as the masses. Disposal: after the copper cools, throw it into the trash can – wipe out the crucible with a dry paper towel.

Reaction 2:Obtain a 3 cm piece of magnesium ribbon. Clamp the magnesium with a pair of crucible tongs. Ignite the magnesium in a Bunsen burner flame and collect the ashes on a watch glass. Do not look directly at the magnesium while it burns. Disposal: throw ashes in trash can after it has cooled down.

Reaction 3:Obtain another 3 cm piece of magnesium. Add 5-10 mL of 3.0 M hydrochloric acid (HCl) to a small test tube in a test tube rack. Add the magnesium to the acid. Using a test tube clamp, invert a second test tube (as shown in the figure below) over the mouth of the reaction test tube and collect the gas being produced. Keep the test tube inverted and test the collected gas by inserting a flaming splint. Record your results. Disposal: after the Mg has reacted completely with the HCl, the solution can go down the sink with lots of water.

Reaction 4:Obtain one scoop of ammonium carbonate, (NH4)2CO3, and place it into a small test tube. Clamp the test tube and heat it in a Bunsen burner. While the test tube is heating, touch a piece of cobalt chloride paper to the mouth of the test tube and remove it. Smell the test tube using the proper wafting technique. Hold a flaming splint in the test tube and record the results of each test. Record.Disposal: any solid remaining in test tube may be rinsed down the sink with water.

Reaction 5:Measure 10 mL of hydrogen peroxide and add to a test tube. Add a very small quantity (tip of spatula) of manganese dioxide, MnO2, (catalyst) to the test tube. Hold a glowing splint inside the mouth of the test tube. Hold a piece of cobalt chloride paper to the mouth of the test tube. Record results.Disposal: place both into the trash.

Reaction 6:Add 1 drop of potassium iodide, KI, and 1 drop of lead (II) nitrate, Pb(NO3)2, to a watch glass. Record the results. Disposal: wipe the watch glass with paper towel and throw paper towel in trash. Do not put it into the sink. Be sure to wash your hands well with soap and water.

Reaction 7:Place two scoops of copper (II) carbonate, CuCO3, into a drylarge test tube. Insert a stopper with a glass bend in the test tube. Clamp the test tube to a ring stand at an angle so that the flame will touch the bottom of the test tube only. Fill a small test tube approximately half way with limewater. Position this test tube so that the end of the glass bend is in the test tube and is submerged in the limewater. Light the Bunsen burner and heat the solid in the large test tube. Observe any changes in the limewater. Disposal: once product cools, place in the trash can, clean test tube; place limewater into the sink with lots of water.

Test Results
Reaction / Observations / Cobalt
Chloride / Splint / Odor / Limewater
  1. Burning Cu
/ Appearance Before:
Appearance After:
Initial Mass:
Final Mass:
  1. Burning Mg
/ Appearance Before:
Appearance After:
  1. Mg and HCl
/ Before:
During:
After: / Flaming splint
  1. Heating (NH4)2CO3
/ Before:
During:
After: / Flaming splint
  1. H2O2
/ Before:
During:
After: / Glowing splint
  1. KI and Pb(NO3)2
/ Before:
After:
  1. Heating CuCO3
/ Before:
After:

Questions:

1. Complete and Balance each equation using the test results above. Indicate the reaction type (synthesis, S,

decomposition, D, single replacement, SR, double replacement, DR, or combustion, C on the line provided.

Reaction 1: type:______

Reaction 2:type:______

Reaction 3:type:______

Reaction 4:type:______

Reaction 5:type:______

Reaction 6:type:______

Reaction 7:type:______

2. Write complete, balanced equations for each of the following. Identify the type (S, D, SR, DR, C):

______a. When potassium bromate is heated, it decomposes into potassium bromide and a gas that reignites a

glowing splint.

______b. Sodium metal reacts violently with water to produce sodium hydroxide and a gas that pops in the

presence of a flame.

______c. When calcium hydroxide is heated, it decomposes into calcium oxide and a substance that will turn

cobalt chloride paper pink.

______d. The Bunsen burner uses methane gas, CH4. It burns in the presence of O2 and produces a

substance that will extinguish a flaming splint and a substance that turns cobalt chloride paper pink.

______e. Iron metal will react with oxygen gas in the air to produce rust, iron (III) oxide.

______f. When you mix baking soda, sodium bicarbonate, with vinegar, acetic acid, they will react violently

to form sodium acetate, and a gas that extinguishes a burning splint and a substance that turns

colbalt chloride paper pink.

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