Meyer_DE_CH_5.4 & 5.5_Chemical Equilibrium & Reaction Rate

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27 questions

Background Knowledge

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Equilibrium Constant (5.4_1)

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Le Chatelier's Principle (5.4_2)

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Solubility Product Constant (5.4_3)

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Factors that Influence Reaction Rate (5.5_1)

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Rate Laws (5.5_2)

Meyer_DE_CH_5.4 & 5.5_Chemical Equilibrium & Reaction Rate

Meyer_DE_CH_5.4 & 5.5_Chemical Equilibrium & Reaction Rate

What do you already know about chemical reactions?

Classify the following equations as balanced or unbalanced.

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.

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

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:

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

HNO2(aq) ⇄ H+(aq) + NO2-(aq)

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

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

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?

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.

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?

Which of the following statements about catalysts is NOT true?

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

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

What do you already know about chemical reactions?

Classify the following equations as balanced or unbalanced.

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.

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

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

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

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:

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

HNO2(aq) ⇄ H+(aq) + NO2-(aq)

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 is used to describe the shift in equilibrium that occurs when a system experiences changes in:

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

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?

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.

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?

Which of the following statements about catalysts is NOT true?

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

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

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

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

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.

Meyer_DE_CH_5.4 & 5.5_Chemical Equilibrium & Reaction Rate

Meyer_DE_CH_5.4 & 5.5_Chemical Equilibrium & Reaction Rate

What do you already know about chemical reactions?

Classify the following equations as balanced or unbalanced.

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.

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

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:

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

HNO2(aq) ⇄ H+(aq) + NO2-(aq)

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

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

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?

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.

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?

Which of the following statements about catalysts is NOT true?

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

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

What do you already know about chemical reactions?

Classify the following equations as balanced or unbalanced.

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.

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

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:

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

HNO2(aq) ⇄ H+(aq) + NO2-(aq)

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 is used to describe the shift in equilibrium that occurs when a system experiences changes in:

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

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?

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.

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?

Which of the following statements about catalysts is NOT true?

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

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

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

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

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.

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.

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:

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.

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:

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.

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.