Lab report A bagged Chemical Reaction PDF

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A Bagged Chemical Reaction Purpose - Observe the changes associated with a chemical reaction including heat changes, changes in an indicator, bubble of gas released. Determine which compounds are reactants and which are products, through the use of a chemical equation. Use indicators in order to identify whether a solution is acidic or basic.

Introduction - Chemical reactions occur when molecules come together to form new products. In our bodies and environments, chemical reactions occur continuously to help run our lives. Chemical reactions can be identified by a chemical equation in which reactants and products are characterized by chemical symbols. All chemical reactions are accompanied by a change in energy. Some reactions release energy to their surroundings and are called exothermic. Some reactions absorb heat from their surroundings which is called endothermic.

Procedures 1.

2.

3.

4. 5.

In a Ziploc bag, place 2 tablespoons of sodium bicarbonate and a film-canister (30 ml) with 3 drops of the phenol red indicator added to the water. Place canister in the bag in the upright position. Squeeze the excess air and seal the bag. Spill the water into the bag and record observations in Data Table 1. In another Ziploc bag add 1 tablespoon of calcium chloride and add the same amount of water as in the previous step but without the phenol red indicator. Repeat procedure in step 1. Record observations in Table 1 In another Ziploc bag, add 2 tablespoons of calcium chloride into one corner of the bag twist off the corner to separate chemical from the rest of the bag and tie. Into the opposing corner of the bag, add 2 tablespoons of sodium bicarbonate and twist off the corner to separate from the rest of the bag and tie. Squeeze the excess air and seal the bag.

A Bagged Chemical Reaction 6.

Carefully untwist the 2 corners (if using rubber bands, use scissors to cut them careful not to cut the bag) while the partner holds both corners apart 7. Release both corners and allow all three chemicals to mix. Quickly observe any immediate changes in the corners. Record all your observations in Table 1 8. In a fourth bag repeat steps #3-8 but this time with 3 drops of the phenol red indicator to the water. Record all your observations in Table

Data Table Physical or Production Chemical of gas Change

Color Change

Temperatu re Change

NaHCO3 in water + Indicator

Chemical

Carbon Dioxide

It turned blue

Endothermic Turned Cold

CaCl2 in water

Chemical

Carbon Dioxide

Clear

Exothermic Turned Warm

NaHCO3 + CaCl2 in water

Chemical

Carbon Dioxide

White

Endothermic Remained Cold

NaHCO3 + CaCl2 with water + Indicator solution

Chemical

Carbon Dioxide

Green

Endothermic Cold

Observation 1. Steps 1,2,3,4, and 8. This is because they all include a characteristic of utilizing chemicals. 2. The change in color or bubbles forming. 3. Process 2 is exothermic because it released heat into its surroundings. 4. Process 1,3,4 is endothermic because they absorbed heat from its surroundings.

A Bagged Chemical Reaction Conclusion’ 1. To indicate whether each chemical solution was acidic or basic. 2. 2NaHCO3+CaCl2 2NaCl+Ca(HCO3)2 3. Sodium Bicarbonate. Calcium Chloride, Sodium Chloride, Calcium Bicarbonate 4. Carbon Dioxide. By evaluating the chemical equation with a double replacement reaction. 5. The energy change could be originated in the air as a gas. 6. The law of conservation of energy...