1. 1 Cu2+ (aq) + 4 Cl- (aq) ⇌ 1 [CuCl4]2–(aq) which reaction shifted the chemical...
1.
|
1 |
Cu2+ (aq) + |
4 |
Cl- (aq) ⇌ |
1 |
[CuCl4]2–(aq) |
which reaction shifted the chemical equilibrium towards the forward direction? Which reaction shifted the chemical equilibrium towards the reverse direction? Explain your reasoning for both using Le Châtelier’s principle.
2. How does the temperature affect the copper(II) chloride equilibrium? Use Le Chatelier’s principle to explain whether the forward reaction is considered an exothermic or endothermic reaction.
Homework Answers
1. Incomplete question.
2. This reaction is exothermic this is because here spontanity is decreased means DS<0 because ions bind together to form a compound. And in Gibbs energy equation DG = DH -TDS (D = Change)
Since DS <0 means TDS will be +ve and DG = 0 since equilibrium is there so to make if 0 DH must be -ve whic h signify that reaction is exothermic.
So on heating or increasing the temprature the reaction will shift towards reactant backward direction.
Add Answer to:
1.
1
Cu2+ (aq) +
4
Cl- (aq) ⇌
1
[CuCl4]2–(aq)
which reaction shifted the chemical...
Determine if the system shifted toward reactants or products for each of the changes. Explain how...
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Question 1
Glucose metabolism can be represented by the following chemical
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C6H12O6(aq)+6O2(g)6CO2(g)+6H2O(l)
H for the
reaction is -2837 kJ/mole.
Is this reaction endothermic or exothermic?
Write an expression for the equilibrium constant for this
reaction.
Given that the value of the equilibrium constant is very large,
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Le Chatelier's Principle 3. For Part Ill, use Le Châteller's Principle to explain the colour changes observed in test tubes 2 and 3 upon the addition of HC and A . Also, explain the observed colour changes in the test tubes placed in hot and cold water. (4 marks) Test Tube 2: Test Tube 3: Hot Water bath: Cold Water bath: Extension: 1. NaCl(aq) + HCl(aq) = NaCl(aq) + H2O + Cl2(g) When the above system is cooled, gas bubbles...
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Question 1
Glucose metabolism can be represented by the following chemical
reaction:
C6H12O6(aq)+6O2(g)6CO2(g)+6H2O(l)
H for the
reaction is -2837 kJ/mole.
Is this reaction endothermic or exothermic?
Write an expression for the equilibrium constant for this
reaction.
Given that the value of the equilibrium constant is very large,
would you expect this reaction to be fast or slow?
Explain the effect on equilibrium of
Increasing temperature
Increasing pressure by decreasing the volume
Decreasing concentration of oxygen
Increasing the concentration of...
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