Which has the most entropy?

They all have the same entropy.

Which one of the following processes produces a decrease in the entropy of the system?

dissolving of solid KCl in water

mixing of two gases into one container

A reaction has the following thermodynamic data. Which of the following statements is true? ΔH° = -75.2 kJ/mol ΔS° = 53.4 J/mol · K

The reaction is thermodynamically favorable at all temperatures.

The reaction is never thermodynamically favorable.

The reaction is thermodynamically favorable at high temperatures.

The reaction is thermodynamically favorable at low temperatures.

If two objects have different temperatures, heat will flow from the warmer object to the cooler one UNTIL ____________

they both have an equal temperature.

one reaches a temperature of zero.

How do the concentrations of Solution X and Y (in the picture below) compare?

They have the same concentration.

Solution X has a greater concentration.

Solution Y has a greater concentration.

There is no way to determine the answer.

The phase changes B → C and D → E are not associated with temperature increases because the heat energy is used to __________.

increase distances between molecules

rearrange atoms within molecules

increase the velocity of molecules

If the equilibrium product to react ratio (K) is 4.5 x 10^ ⁻¹¹ for a reaction, which of the following would be true?

Reactants are favored at equilibrium

Products are favored at equilibrium

Reactants and products are equally favored at equilibrium

Consider the reaction below. The equilibrium constant at 400ºC is K=0.50. Suppose we make a mixture with the following concentrations: [NH₃] = 1.0M, [N₂] = 1.0M, [H₂] = 1.0M. Which direction will the reaction shift to reach equilibrium?

No shift will occur because this reaction is already at equilibrium.

A container filled with carbon dioxide and carbon tetrafluoride is allowed to react and reach equilibrium. If more CO₂ is added after the system reaches equilibrium, what will happen?

The forward reaction will speed up until equilibrium is achieved again.

The system will have a new equilibrium constant, K.

The reaction will shift to the left.

The forward reaction will speed up forever!!!

How does increasing the temperature affect the solubility of solids in liquids?

Increasing temperature increases the solubility of solids

Increasing temperature decreases the solubility of solids

Increasing temperature has no effect on the solubility of solids

Which of the following correctly describes a reaction system at equilibrium?

Reactions continue to occur, but there is no detectable changes in concentration of reactants or products.

All reactions stop at equilibrium and no detectable changes can be made.

Reactions continue to occur, and concentrations of reactants and products can increase or decrease.

Reactions continue to occur, decreasing concentrations of reactants and increasing concentrations of the products.

Chem 2023 Spring Semester Review

Authored by Sally Dew

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12th Grade

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MULTIPLE CHOICE QUESTION

1 min • 1 pt

Breaking bonds ________ energy.

requires

releases

transfers

destroys

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which of following is NOT true according to the laws of thermodynamics.

Energy can be transferred from one form to another, but can not be created or destroyed

The entropy of the universe is always increasing.

The energy of the universe is always increasing.

Heat will flow from hot to cold until there thermal equilibrium is reached.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which of the following is true about the reaction pictured below?

I and III

II and IV

II and III

I and IV

MULTIPLE CHOICE QUESTION

1 min • 1 pt

What is the estimated energy required to break the bonds at the beginning of the reaction pictured?

80 kJ

160 kJ

240 kJ

280 kJ

MULTIPLE CHOICE QUESTION

1 min • 1 pt

How much heat is released when 125 g of sulfur dioxide are produced according to the following reaction: S + O₂ → SO₂ H = -296 kJ

-577 kJ

-296 kJ

-1156 kJ

-32 kJ

MULTIPLE CHOICE QUESTION

1 min • 1 pt

A 28.4 g sample of metal is heated to 39.4°C, then is placed in a calorimeter containing 50.0 g of water. Temperature of water increases from 21.00°C to 23.00°C. What is the specific heat of the metal? (q=cmΔT, specific heat of water = 4.18 J/g°C)

4.18 J/g°C

0.897 J/g°C

1.345 J/g°C

0.374 J/g°C

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Liquid water turns to ice. Is this process endothermic or exothermic? Choose the best answer.

Endothermic. The water absorbed heat and got colder, thereby forming ice.

Endothermic. Energy in the form of heat was given off by the water, which became colder and formed ice.

Exothermic. The water released thermal energy, slowing down the water molecules so that solid ice formed.

Exothermic. Heat was absorbed by the water, moving its molecules faster so that they condensed on an object and formed ice.

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Chem 2023 Spring Semester Review

Breaking bonds ________ energy.

Which of following is NOT true according to the laws of thermodynamics.

Which of the following is true about the reaction pictured below?

What is the estimated energy required to break the bonds at the beginning of the reaction pictured?

How much heat is released when 125 g of sulfur dioxide are produced according to the following reaction: S + O₂ → SO₂ H = -296 kJ

A 28.4 g sample of metal is heated to 39.4°C, then is placed in a calorimeter containing 50.0 g of water. Temperature of water increases from 21.00°C to 23.00°C. What is the specific heat of the metal? (q=cmΔT, specific heat of water = 4.18 J/g°C)

Liquid water turns to ice. Is this process endothermic or exothermic? Choose the best answer.

Which has the most entropy?

Which one of the following processes produces a decrease in the entropy of the system?

The thermodynamic quantity that expresses the degree of disorder in a system is __________.

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