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Meyer_DE_CH_5.4 & 5.5_Chemical Equilibrium & Reaction Rate

Last updated over 2 years ago
27 questions
Background Knowledge
1

What do you already know about chemical reactions?

Required
1

Classify the following equations as balanced or unbalanced.

  • Balanced
  • Unbalanced
Required
1

How much do you know about reactions?

Some reactions are endothermic and absorb heat energy, and other reactions are exothermic and release heat energy. Think about the following scenarios and sort them into endothermic or exothermic reactions.

  • baking bread
  • making ice
  • cooking an egg
  • melting ice
  • burning wood
  • evaporation of water
  • burning leaves
  • condensation
  • Endothermic
  • Exothermic
Required
1
A chemical reaction that can only proceed in a single direction is considered _______. A chemical reaction that can proceed in either the forward or reverse direction is known as a _______ reaction.
Required
1

If you totaled up the mass of the reactants, they would _____ the mass of the product.

Required
2
The products of the reaction is __________ .
The reactants of the reaction is _______ (a metal) and _______ (a nonmetal).
The coefficient of O2 is ______ .
The coefficient of Fe2O3 is ______ .
Other Answer Choices:
3
1
2
FeO2
Fe2O3
O2
4
Fe
0
Equilibrium Constant (5.4_1)
Required
1
In irreversible reactions, all of the _______ is changed to _______ . However, not all chemical reactions use up all of the reactants. When a reaction is at _______ , quantities of both reactants and products remain present.
Required
1

Entropy is a measure of the "disorder" of a system. What is the change in entropy in an ideal reversible chemical reaction.

Required
1

The change in entropy is positive, this means that entropy _____.

Required
1
When a chemical reaction is at equilibrium, the concentration of reactants and products does not change. A constant value that describes this reaction is the equilibrium constant, or Keq.

For the reaction, aA + bB ⇄ cC + dD , the equilibrium constant, Keq, is described as _____.
Other Answer Choices:
[A]a
[B]b
[C]c
[D]d
Required
1

Solid substances and liquid water are not included in equilibrium calculations. This is due to the structure of the particles in both liquids and solids.

Which is the correct equilibrium constant for the following equation:

Required
1

When a reaction is at equilibrium, the concentrations of reactants and products are always equal.

Nitric acid dissociates in water according to the following equilibrium equation:

HNO2(aq) ⇄ H+(aq) + NO2-(aq)

Required
1
1.0 mol HNO2 is dissolved in water to make 0.50 liters of solution. Construct an ICE table to represent the problem.
Other Answer Choices:
0
2.0 - x
x - 2.0
0 + x
-x
2.0 + x
x
-x
0
0 + x
x
Required
1

Use the ICE table and chemical equation from the previous question to calculate the concentrations of H+ Ions that will be present at equilibrium.
The equilibrium constant, Keq, at 25°C,
for this is 4.0 × 10−4.

Le Chatelier's Principle (5.4_2)
Required
1
Additional reactant is added to the system.
System response: __________
Required
1
Products are removed from the system as they are produced.
System response: __________
Required
1
The air pressure above an aqueous system at equilibrium is increased.
System response: __________
Required
1

Le Chatelier’s Principle is used to describe the shift in equilibrium that occurs when a system experiences changes in:

Required
1

Which of the following statements will increase the amount of product that is created in a chemical reaction?

Solubility Product Constant (5.4_3)
Required
1
If the ion product is __________ Ksp, then a precipitate will not form.
If the ion product from the mixture is __________ Ksp, then a precipitate will form.
Required
1

The solubility constant of MnS is 2.3 ×10−13 at 25°C. What is the concentration of sulfide ions in a saturated solution of MnS at equilibrium?

Required
1

Iron carbonate, FeCO3, is added to water until the saturation point is reached. What concentration of carbonate ion, CO32-, is present in this solution? The solubility constant for FeCO3 is 2.1×10−11 at 25°C.

Required
1

The solubility constant of Ba(OH)2 is 5.0 ×10−3 at 25°C. Calculate the equilibrium concentration of hydroxide ions in a saturated solution?

Factors that Influence Reaction Rate (5.5_1)
Required
1

Which of the following statements about catalysts is NOT true?

Required
1

Choose one or more of the following statements that can lead to a chemical reaction to occur faster.

Required
1
A _______ will reduce the amount of activation energy needed for a reaction to occur. The use of an _______ will decrease reaction rate.
Required
1

Choose one or more of the following statements that can lead to a chemical reaction to occur faster.

Rate Laws (5.5_2)