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Exp 9 Chem 14.1

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Jenishia Romano

on 19 March 2013

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Transcript of Exp 9 Chem 14.1

Chemical Equilibrium Experiment no. 9
Chemical equilibrium applies to reactions that occur in both directions. The laws of chemical equilibrium describe the direction in which a chemical reaction will go, either forward or backward.
Chemical reactions do not generally go into completion.
The state of equilibrium is reached if the rate of the formation of the reactants is equal to the rate of the formation of the products.
It is dynamic and involves the continuous and simultaneous formation of products from the reactants and reactants from products. Introduction To evaluate the effect of change in concentration and change in temperature on the equilibrium system Objectives Materials: Methodology Reagent Results Fe 3+, CNS-, Na+, F-, Ag+, NO3- Guide Questions Alyssa Gayle P. Merilles
Jenishia Maria A. Romano To explain the effect of these changes on the equilibrium system To interpret the results based on the Le Chatelier's principle 0.1 M Fe(NO3)3
0.1 M KCNS
0.1 M KCl
0.1 M AgNO3
NaF crystals
ice water
100 ml beaker
1 spot plate 20 drops of 1 M Fe(NO3)3 solution + 20 drops of 1 M KCNS solution + 7 ml water on a 10 ml test tube Methodology Place 10 drops of the solution prepared in #1 on 8 holes of spot plate Reagent (10 drops) 5+7= distilled water
0.1 Fe(NO3)3
0.1 M KCNS
0.1 M KCl
0.1 M AgNO3
a pinch of NaF 1
2
3
4
5
6 Methodology Add 10 drops of distilled water to test tubes 7 and 8 Place test tube 7 in ice water Heat test tube 8 over a hot plate Observation Direction of shift 0.1 M Fe(NO3)3
0.1 M KCNS
0.1 M KCl
0.1 M AgNO3
Pinch of NaF
Increase in temp
Decrease in temp forward
forward
no shift
backward
backward
backward
forward darker
darker
no change
lighter
lighter
lighter
darker 5+7= (cc) image by anemoneprojectors on Flickr 1. Explain your observations on the basis of Le Chatelier's principle. Based on Le Chatelier's principle, the experiment has undergone changes in conditions which resulted in the change in the shifts of the reactions. 2. Which species (ions) in the added reagents are effective in altering the state of the system? 3. Is the reaction endothermic or exothermic? The color of the solution turned lighter as the temperature was increased therefore, the reaction was exothermic. Fe3+ + CNS- FeCNS2+
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