Chem Lab Exam Ch. 7-12 Questions and Correct Answers
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Course
Chem
Institution
Chem
What parts are present in every chemical equation?
~ -At least one reactant
-At least one product
-An arrow
Identify the correct equation and net ionic equation for the reaction between aqueous
hydrochloric acid and aqueous sodium carbonate.
~ ~2HCl(aq)+Na2CO3(aq)⟶2NaCl(aq)+H2O(l)+CO2(g)
...
Chem Lab Exam Ch. 7-12 Questions
and Correct Answers
Which statement is true about a chemical reaction at equilibrium?
✓✓~ The forward reaction rate is equal to the reverse reaction rate.
Consider the two reactions of iron ions, one with thiocyanate (SCN−) ions and one
with chloride (Cl−) ions.
✓✓~ If you create an equilibrium mixture from Fe3+ and SCN− ions, adding Cl− ions will shift the
iron-thiocyanate equilibrium to the reactant side because it removes iron from the iron-thiocyanate
equilibrium mixture.
Determine whether each description corresponds to an endothermic reaction or an
exothermic reaction.
✓✓~ -Heat is a reactant in the reaction. (Endothermic)
-The reaction mixture feels cool from the outside. (Endothermic)
-The reaction mixture feels warm from the outside. (Exothermic)
-Heat is a product in the reaction. (Exothermic)
When any reversible reaction is at equilibrium, what conditions are necessarily true?
✓✓~ -Reactants and products are both present in the reaction mixture.
-The rate of the forward reaction equals the rate of the reverse reaction.
-The amounts of reactants and products has stopped changing.
, According to Le Châtelier's Principle, heat applied to an exothermic reaction will shift
the reaction towards _____________. Heat applied to an endothermic reaction will
shift the reaction towards _____________.
✓✓~ the reactants , the products
Consider the equilibrium system of cobalt complexes.
Co(H2O)62+(aq)+4Cl−(aq)−⇀↽−CoCl42−(aq)+6H2O(l)
The Co(H2O)62+(aq) complex is pink and the
CoCl42−(aq) complex is light blue.
Determine what each color observation means about changes made to the system at
equilibrium.
✓✓~ -The solution changes from light blue to pink. >>The change shifted the equilibrium to the
reactant side.
-The solution stays light blue after adding a chemical. >>The change did not shift the
equilibrium system.
-The solution changes from pink to light blue. >>The change shifted the equilibrium
to the product side.
A change in temperature can shift an equilibrium system.
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