1.) Consider the following reaction: A + 2 B + Heat C + 3 D. Based on the observ
ID: 549651 • Letter: 1
Question
1.) Consider the following reaction: A + 2 B + Heat C + 3 D. Based on the observations in the experiment, explain how it would be possible to shift this reaction in the forward direction.
2.) Consider the following reaction: Z + 4 Y Q + 2 S, H = -value. Again, based on experimental observations, explain how it would be possible to reduce the amount of Q in the reaction.
3.) If a suitable catalyst had been added to the reactions studied in the experiment, how would this have affected the results of the tests carried out?
The experiment information:
Stock solution: 6 drops of 0.10M KSCN, 6 drops of 0.20M Fe(NO3)3, and 6 ml of water mixed
place 10 drops of stock solution in each well
added 3 drops of 0.20M Fe(NO3)3 in well plate 2 and 3 drops of 0.10M KSCN in well plate 3 and in both cases the reacton equilibrium shifted to the right.
added 3 drops of 6M NaOH and 3 drops and 3 drops of 6M HNO3 the reaction equilibrium shifted to the left.
when heated the reaction became exothermic
when cooled the reaction became endothermic
Explanation / Answer
Answer 1)
Given thermochemical change,
A + 2 B + Heat C + 3 D
We supposed to shift reaction in the forward direction and we are asked to suggest something to do so.
This question is based on Le Chatelier's principle states that,
When any of the constrains like change in T, P, V concentration etc imposed on system in an equilibrium then system tries to nulify that constrain by shifting an equilibrium in the direction which nulifies it.
By observing given chemical equation it's clear that its an endothermic reaction (i.e. reactants absorbs heat to form product).
Simply by increasing temperature of reaction will provide excess heat to the reactant side to nulify it reactants will consume more heat and will form products.
This makes the reaction more in the forwarding direction.
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