Which K value below is consistent with an equilibrium system in which the reactants are favored?

1)  An equilibrium constant with a value of 8.0 × 106 indicates that at equilibrium ________.

 

A) the reactants are favored

 

B) the products are favored

 

C) approximately equal concentrations of reactants and products are present

 

D) there are more reactants present than products

 

 

 

2)  Which K value below is consistent with an equilibrium system in which the reactants are favored?

 

A) K = 1

 

B) K = 1.8 x 103

 

C) K = 3.7 x 10–8

 

D) K = 500

 

 

 

3)  Which statement about catalysts is NOT true?

 

A) A catalyst increases the rate of a chemical reaction.

 

B) A catalyst lowers the activation energy of a chemical reaction.

 

C) A catalyst lowers the ΔH of a chemical reaction.

 

D) A catalyst is recovered unchanged in the reaction it catalyzes.

 

 

 

4)  Which of the following is ALWAYS necessary for a chemical reaction to occur between two reactants, A and B?

 

A) Equal amounts of A and B must be present

 

B) A and B must be present in the same physical state

 

C) The reaction must be carried out at a temperature higher than room temperature

 

D) A and B must collide with the proper orientation and with a certain minimum amount of energy

 

In each of the following questions, identify which way (to the left or to the right) does equilibrium shift to relieve the described applied stress:

 

5)  Consider the following reversible reaction at equilibrium: CO(g) + Cl2(g) ? COCl2(g). If chlorine gas is added to the equilibrium system, how is the stress relieved?

 

 

 

 

 

 

 

6)  Consider the following reversible reaction at equilibrium: C6H12O6 (aq) + 6 O2(g) ? 6 CO2(g) + 6 H2O(l).  If oxygen gas is removed from the equilibrium reaction vessel, how is the stress relieved?

 

 

 

7)  Consider the following reversible reaction at equilibrium: C6H12O6 (aq) + 6 O2(g) ? 6 CO2(g) + 6 H2O(l).  Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?

 

8)  Label each identified lettered component of the energy diagram for the arbitrary chemical reaction below:

 

A)

 

 

 

B)

 

 

 

C)

 

 

 

D)

 

 

 

E)

 

 

 

 

 

Problem Solving (Show your work):

 

9)  What is the symbolic expression for the equilibrium constant for the reaction:

 

2 C2H6(g) + 7 O2(g) ? 4 CO2(g) + 6 H2O(g)?

 

 

 

 

 

 

 

 

 

10)  What is the gas phase chemical reaction that corresponds to the equilibrium constant expression shown below? 

 

 

 

 

 

11)  Consider the reaction: N2(g) + O2(g) ? 2 NO(g). If [N2] = 0.520 M, [O2] = 0.0662 M, and [NO] = 0.00956 at equilibrium, calculate the value of K and describe the physical/chemical interpretation of this K value.

 

12) Watch the following video that illustrates a series of experimentsthat demonstrate Le Chatelier’s principle:https://www.youtube.com/watch?v=ZOYyCTvLa9E

 

In this video, you will observe several examples of external stresses that act upon the equilibrium chemical reaction:

 

Feaq+3+SCNaq-1?FeSCNaq+2

 

Each stress will serve to either add or remove reactant or product.

 

A)  Describe what happens when iron nitrate or potassium thiocyanate (reactant) are added to the control tube? Describe your observation in the context of Le Chatelier’s principle.

 

B)  Describe what happened when sodium hydroxide was added to the control tube?  Does the addition of sodium hydroxide add or remove a reactant or product?  If so, clearly state the effect of adding sodium hydroxide and how equilibrium shifts to relieve this stress.

 

C)  Similarly, describe what happened when potassium chloride was added to the control tube?

 

D)  Next, describe what happened when silver nitrate was added to the control tube?

 

E) Lastly, describe what happens when Mercury (II) Nitrate was added to the control tube?

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