This document describes an experimentation in chemistry lesson. Students will perform various experiments involving physical and chemical changes. They will observe the burning of candles, the mixing of substances like vinegar and baking soda, and the dissolving of solids like salt and sugar. The goal is for students to understand the differences between physical and chemical changes and be able to classify changes as one or the other. They will also discuss the requirements for burning and the products of combustion.
One of a series of presentations giving an overview of the crime scene, forensics and tasking. I initally created these as part of a self teach process
The rate of reaction is the speed at which a reaction proceeds. The factors that affect the rate of a chemical reaction are : nature of reactants, temperature, concentration, size of particle and catalyst.
UV/Vis spectroscopy is routinely used in analytical chemistry for the quantitative determination of different analytes, such as transition metal ions, highly conjugated organic compounds, and biological macromolecules. Molecules containing bonding and non-bonding electrons undergo electronic transitions and absorb energy in the form of ultraviolet or visible light to excite these electrons to higher anti-bonding molecular orbitals.
Classic, mini chemistry experiments- some require materials typically found in a high school chemistry lab, while others are extremely simple. Very straightforward!
One of a series of presentations giving an overview of the crime scene, forensics and tasking. I initally created these as part of a self teach process
The rate of reaction is the speed at which a reaction proceeds. The factors that affect the rate of a chemical reaction are : nature of reactants, temperature, concentration, size of particle and catalyst.
UV/Vis spectroscopy is routinely used in analytical chemistry for the quantitative determination of different analytes, such as transition metal ions, highly conjugated organic compounds, and biological macromolecules. Molecules containing bonding and non-bonding electrons undergo electronic transitions and absorb energy in the form of ultraviolet or visible light to excite these electrons to higher anti-bonding molecular orbitals.
Classic, mini chemistry experiments- some require materials typically found in a high school chemistry lab, while others are extremely simple. Very straightforward!
Classic, mini chemistry experiments- some require materials typically found in a high school chemistry lab, while others are extremely simple. Very straightforward!
Lab 9 Chemical Reactions IIPre-lab Questions1. What is a limi.docxsmile790243
Lab 9: Chemical Reactions II
Pre-lab Questions
1. What is a limiting reagent?
2. A student used 7.15 g of CaCl2 and 9.25 g of K2CO3 to make CaCO3. The actual yield was 6.15 g of CaCO3. Calculate the limiting reagent and the percent yield.
Experiment: Synthesis of Garden Lime
Procedure
**Take photographs of your experiment set up and your results. Submit them with your laboratory report.**
1. Table 1 provides an example set of data for 1.0 g CaCl2.
2. For Trial 1, weigh into a 250 mL beaker the amount of calcium chloride (CaCl2) shown in Table 1. Record the exact mass you weigh out in the Trial 1 column of the Data section.
3. Measure 50.0 mL of distilled water into a 100 mL graduated cylinder. Pour the water into the 250 mL beaker with the calcium chloride.
4. Stir the solution with a stirring rod until all of the calcium chloride is dissolved.
5. Weigh out 2.5 g of potassium carbonate (K2CO3) in a 50 mL beaker. Record the exact mass in the Data section.
6. Measure 25.0 mL of distilled water into a 100 mL graduated cylinder. Add the water into the 50 mL beaker containing the potassium carbonate.
7. Stir the potassium carbonate in the distilled water with a stirring rod until it is all dissolved.
8. Pour the K2CO3 solution into the 250 mL beaker that has the CaCl2 solution. Rinse the beaker that contained the K2CO3 with a few mL of water and add this to the CaCl2 solution. Stir the mixture.
9. As soon as the reaction begins, record your observations in the Data section. Continue stirring until you see no more precipitate forming.
10. Set up the funnel in the Erlenmeyer flask as shown in Figure 2.
HINT: Do NOT begin filtering yet!
11. Zero the scale and weigh a piece of filter paper and a watch glass. Record the masses of both items in the Data section.
12. Prepare a filtering funnel as shown in Figure 2: fold a piece of filter paper in half twice to make quarters, and open the paper to make a small cone (three quarters are open on one side and one quarter is on the opposite side). Place the paper cone into the funnel and hold it in place with your fingers. Pour a small amount of distilled water through the paper to secure it inside the funnel.
13. Filter the mixture by pouring it into the filter paper in the funnel. Use the stirring rod and distilled water in a wash bottle to transfer the entire solid into the filter paper.
HINT: For best results, be sure to transfer all of the precipitate into the filter paper. Use a rubber policeman if it is available to help with the transfer.
14. Rinse the remaining solid in the filter paper twice with distilled water from a wash bottle to rinse off excess sodium chloride (NaCl). After all the liquid has filtered through, rinse the product with approximately 5 mL of ethanol to aid in its drying. Allow the ethanol to completely finish filtering through the paper.
15. Remove the filter paper carefully so as to not lose any product. Gently unfold the filter paper and lay it flat on the pre-weighed wat ...
phychem1phychem2Lab 9 Chemical Reactions IIPre-lab Qu.docxmattjtoni51554
phychem1phychem2
Lab 9: Chemical Reactions II
Pre-lab Questions
1. What is a limiting reagent?
2. A student used 7.15 g of CaCl2 and 9.25 g of K2CO3 to make CaCO3. The actual yield was 6.15 g of CaCO3. Calculate the limiting reagent and the percent yield.
Experiment: Synthesis of Garden Lime
Procedure
**Take photographs of your experiment set up and your results. Submit them with your laboratory report.**
1. Table 1 provides an example set of data for 1.0 g CaCl2.
2. For Trial 1, weigh into a 250 mL beaker the amount of calcium chloride (CaCl2) shown in Table 1. Record the exact mass you weigh out in the Trial 1 column of the Data section.
3. Measure 50.0 mL of distilled water into a 100 mL graduated cylinder. Pour the water into the 250 mL beaker with the calcium chloride.
4. Stir the solution with a stirring rod until all of the calcium chloride is dissolved.
5. Weigh out 2.5 g of potassium carbonate (K2CO3) in a 50 mL beaker. Record the exact mass in the Data section.
6. Measure 25.0 mL of distilled water into a 100 mL graduated cylinder. Add the water into the 50 mL beaker containing the potassium carbonate.
7. Stir the potassium carbonate in the distilled water with a stirring rod until it is all dissolved.
8. Pour the K2CO3 solution into the 250 mL beaker that has the CaCl2 solution. Rinse the beaker that contained the K2CO3 with a few mL of water and add this to the CaCl2 solution. Stir the mixture.
9. As soon as the reaction begins, record your observations in the Data section. Continue stirring until you see no more precipitate forming.
10. Set up the funnel in the Erlenmeyer flask as shown in Figure 2.
HINT: Do NOT begin filtering yet!
11. Zero the scale and weigh a piece of filter paper and a watch glass. Record the masses of both items in the Data section.
12. Prepare a filtering funnel as shown in Figure 2: fold a piece of filter paper in half twice to make quarters, and open the paper to make a small cone (three quarters are open on one side and one quarter is on the opposite side). Place the paper cone into the funnel and hold it in place with your fingers. Pour a small amount of distilled water through the paper to secure it inside the funnel.
13. Filter the mixture by pouring it into the filter paper in the funnel. Use the stirring rod and distilled water in a wash bottle to transfer the entire solid into the filter paper.
HINT: For best results, be sure to transfer all of the precipitate into the filter paper. Use a rubber policeman if it is available to help with the transfer.
14. Rinse the remaining solid in the filter paper twice with distilled water from a wash bottle to rinse off excess sodium chloride (NaCl). After all the liquid has filtered through, rinse the product with approximately 5 mL of ethanol to aid in its drying. Allow the ethanol to completely finish filtering through the paper.
15. Remove the filter paper carefully so as to not lose any product. Gently unfold the filter paper and lay it flat on t.
Classic, mini chemistry experiments- some require materials typically found in a high school chemistry lab, while others are extremely simple. Very straightforward!
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2. .
Experiment No. 1
Experimentation in Chemistry
Theory:
Chemist (scientists) make a great deal of
experimentation as they apply scientific
methods of study. The greatest part in a
chemist’s activities is spent in experimentation.
3. .
You too, as beginning chemists, will have
to perform experiments that will enable to
solve problems you will encounter in the
study of chemistry.
4. .
When gold and silver alloys are molded or
shaped into fine jewelries, no new substances is
formed. Only a change in physical form (shape)
occurs. Hence, this is called a physical change.
For example, when solid water (ice) is heated, it
first changes to liquid water and finally to steam.
5. .
There is no change in the composition of the
substance, only in the form in which it exists.
Consider the change that takes place when
salt dissolves in water. Even though the form
of salt changes, the composition does not. It
is still sodium chloride (NaCl), but now it is
dissolved in water.
6. .
. A chemical change occurs when new
substances is formed. The new substance have
properties entirely different from those of the
original substances. The original substances are
called reactants; the new substances formed are
called products.
7. .Burning candle is an example of chemical
change. When a candle burns it produces heat,
flame, and soot. Soon the candle disappears,
actually two new substances are formed-
carbon dioxide and water vapor. You do not see
these products because they are lost to the
atmosphere.
8. In this activity, you will perform some
common laboratory techniques in order to
identify the characteristics of physical and
chemical changes.
9. .
.OBJECTIVES:
a) To know what are needed for burning to take
place.
b) To know the products of burning.
c) To know the gases and the particles that makes
up the air.
10. .
d) To differentiate physical changes from
chemical changes
e) To classify some changes as physical and
chemical
32. .
.1. Quickly blow out the candle flame and
quickly relighted the candle at the column of
smoke ½ cm from the wick. Record your
observation. See Figure 1
34. .
2. Move a horizontally held piece of cardboard
quickly down over the flame of a burning
candle. Take note, do not burn the cardboard.
Record your observation.
35. ‘.
3) a) Invert a beaker over a lighted candle.
Take note the time the flask completely
covered the candle and the time the candle
flame is put off. See Figure 2.
Record your observation.
37. .
.b) Relight the candle, invert a smaller beaker
over the lighted candle. Take note again the
candle flame is extinguished.
38. .
.4) Fill a beaker with cold water. Add one (1)
teaspoon of vinegar, then add one teaspoonful of
baking soda. Stir well. Quickly drop the mothballs.
See Figure 3.
Record your observation after a few minutes.
40. .
.5) Place a sheet of crumpled paper inside an
empty glass. Let it rest at the bottom. Put the
glass mouth down into the beaker full of water.
41. .
Push the glass slowly into the water until it
reaches the bottom of the beaker. Get the paper
from the glass. Is the paper wet or dry?
42. .
6) Use a hard-boiled egg with its shell removed.
Light a piece of paper and drop it into an
Erlenmeyer flask or a wide-necked bottle. Place
the egg (sharp end down) on the flask and observe
what happened. See Figure 4.
44. .
.
7) Ignite 2 ml of alcohol in an evaporating dish
Record your observations:
__________________________________
__________________________________
__________________________________
45. .
.8) Allow 2 ml of alcohol to stand in a watch glass
for five minutes. See Figure 5.
Observations:
_____________________________________
_____________________________________
_____________________________________
47. .
9) Place 5 grams of iron fillings in a watch glass
and magnetize.
Record your observations:
______________________________________
______________________________________
______________________________________
48. .
10) Place a small pieces of ice cubes in a beaker
for a few minutes. See Figure 6.
Record your observations:
___________________________________
___________________________________
___________________________________
Record
50. .
’11) Burn a small piece of magnesium ribbon.
See Figure 7.
Record your observations:
____________________________________
____________________________________
____________________________________
52. .
12) Dissolve a pinch of sodium chloride
crystals in 10 ml of water.
See Figure 8.
Record your observations:
___________________________________
___________________________________
___________________________________
54. .
13) Dissolve one spoonful of sugar in 4 spoonful
of vinegar.
Record your observations:
___________________________________
___________________________________
___________________________________
55. .
14) Dissolve one spoonful of baking soda in 4
spoonful of vinegar.
Record your observations:
_________________________________
_________________________________
_________________________________
56. .
For Discussion: Answers to be submitted next
meeting:
1. What are the requirements for burning to take
place?
2. What are the product of burning?
3. What are the gases and particles that makes
up the air?
57. .
4) In procedure 5, is the paper wet or dry? What
is the reason behind?
5) Which of the substances have undergone
chemical changes?
6) Which of the substances have undergone
physical change?
7) Differentiate chemical change from a physical
change.