and Exothermic Experiment no 5 Group no 2 Leader Tara Faye Bayas Members Ann Marjory V Cariño Pearly Ruby Cariaga Kristine Grace Cortez Julius Bryan Cruz Endothermic And Exothermic Reaction ID: 476370
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Slide1
Endothermic
and
Exothermic
Experiment no. 5
Group no. 2
Leader: Tara Faye
Bayas
Members:
Ann Marjory V.
Cariño
Pearly Ruby
Cariaga
Kristine Grace Cortez
Julius Bryan Cruz Slide2
Endothermic And Exothermic ReactionSlide3
INTRODUCTION
Chemical reaction may proceed with a net absorption of energy or with a net release of heat. The energy transaction may include heat, light or electricity. The term ‘endothermic’ and ‘exothermic’ refer to the heat exchange only. Slide4
Endothermic Reaction
The word
endothermic
("within-heating") describes a process or reaction in which the system absorbs
energy
from the surroundings in the form of
heat
. Its etymology stems from the prefix
endo
-
(derived from the Greek word
ένδον
,
endon
, "within") and the Greek word
thermasi
, (meaning “to heat”). The opposite of an endothermic process is an
exothermic
process, one that releases energy in the form of heat. The term
endothermic
was coined by
Marcellin
Berthelot
.
Expressed in a Chemical Equation:
Energy
+ Reactants
→ ProductsSlide5Slide6
The reactants have less potential energy than reactants.
Energy must be input in order to raise the particles up to the higher energy level.Slide7
example of Endothermic reaction
Photosynthesis
is an example of an endothermic reaction. The chlorophyll and pigments in the plant absorb the light energy from the sun's rays, as endothermic reaction is that in which energy is absorbed.Slide8
Exothermic Reaction
Exothermic
is a chemical reaction that releases energy in the form of light or heat. It is the opposite of an endothermic reaction.
Expressed
in a chemical equation:
reactants
→ products + energySlide9Slide10
The reactants have more potential energy than the products have.
The extra energy is released to the surrounding.Slide11
Example of Exothermic reaction
Explosions are examples of exothermic reactions as they release energy to their surroundings.Slide12
Objective
To determine the energy changes that
occur during a certain type of chemical reactionSlide13
Balance
Beaker, 50 mL
Graduated Cylinder, 50
mL
Styrofoam cup/calorimeter
Temperature
Weighing paper
MaterialsSlide14
reagents
Baking Soda(NaHCO3)
1.5 M Citric acid (H3C6H507)
2 M HCL
Magnesium ribbonSlide15
Part 2
Reacting Citric Acid and Baking Soda
1.
Part II
Place
a 150 mL- beaker into the calorimeter as shown in the diagram. Put 30 mL of 1.5 M citric acid into the beaker. Place the temperature sensor into the citric acid solution. Click on “REC” button to begin data recording.
Weigh out 10.0g of baking soda on a piece of weighing paper. After about 20 seconds have elapsed, add the baking soda to the citric acid solution. Gently stir the mixture to ensure complete reaction substances.
Allow the computer to record data until a minimum temperature has been reached and temperature readings begin to increase or let the computer automatically end it after 250 seconds.
Dispose the reaction products and rinse the cup.
Reacting Magnesium and Hydrochloric Acid
Repeat Procedure A using magnesium ribbon ( 5 cm long) instead of baking soda and hydrochloric acid in place of citric acid 1.5 M.
PROCEDURESlide16
Final Temp.
20Initial Temp.
30
Temp. Change
10 C
Final Temp.
30
Initial Temp
25
Temp. Change
-5
Data from: Gr. 4
Citric acid + Baking Soda
Run no. 1
HCL + Mg ribbon
Run no.2
Data and resultSlide17
1. What
type of energy change is associated with the chemical reaction between Citric Acid and Baking Soda?
-chemical
change
.
Endothermic Reaction
With magnesium and Hydrochloric Acid
-Heat
energy.
Exothermic
Reaction
2. How
do the experimental data support the energy changes described?
-Through the heat that we applied , some of the chemicals that we mixed
Data and ResultSlide18
3.What
does a
negative
T value indicates?
it
indicates into a colder
region and it means that the temperature goes down. Therefore the endothermic reaction took place.
4.Described
3 ways to determine that chemical reaction has taken place.
- when the experiment has taken place. The experimental take reaction/ then it bring into a natural reaction
Change in color
Change in odor
Change in temperature
Release of gasSlide19
5. Which
reaction took place at a greater rate? Explain.
The Exothermic Reaction ( Magnesium Ribbon and the Hydrochloric Acid ).
- Shows higher temperature . Slide20
THANK YOU!!!