Free Printable Enthalpy, Entropy, and Gibbs Free Energy

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Enthalpy, Entropy, and Gibbs Free Energy

Total questions: 15

Worksheet time: 14mins

Name

Class

Date

Which reaction has the greatest increase in entropy?

2H₂0 (l) --> 2H_{2 (g)} + O_{2 (g)}

2H₂O(g)--> 2H₂(g) + O₂(g)

H₂O(g) --> H₂O(l)

H₂O(l) H₂O(s)

Which process is accompanied by a decrease in entropy?

boiling of water

condensing of water vapor

subliming of iodine (solid directly to gas)

melting of ice

Systems in nature tend to undergo changes toward

lower energy and less disorder

lower energy and more disorder

higher energy and less disorder

higher energy and more disorder

Given the change of phase:

CO₂(g) —> CO₂(s)

As CO₂(g) changes to CO₂(s), the entropy of the system

decreases

increases

remains the same

Which phase change represents a decrease in entropy?

solid to liquid

gas to liquid

liquid to gas

solid to gas

Identify whether the following result in an increase or decrease in entropy:

Gas --> Liquid --> solid

increase

decrease

Entropy increases from solid, liquid to gas. Why?

Molecular disorder increases

Molecular randomness decreases

Molecules are more energetic

Molecules are more reactive

A reaction has a positive ΔH and a positive ΔS. Which of the following is true?

It will be spontaneous at all temperatures.

It will be nonspontaneous at all temperatures.

It will be spontaneous at low temperatures.

It will be spontaneous at high temperatures.

Two factors that determine the spontaneity of a reaction are:

entropy and free energy

enthalpy and free energy

entropy and enthalpy

endothermic and exothermic

10.

Reactions tend to be spontaneous if they are exothermic.

True

False

11.

This appears on the left side of a chemical formula, and represents how many molecules there are.

An Atom

The Subscript

A Molecule

The Coefficient

12.

1. Given the following information, calculate ΔG⁰ for the reaction below at 25⁰C:

SnCl₄(l) + 2 H₂0(l) → SnO₂(S) + 4HCl(g),

ΔH⁰=133.0 kJ and ΔS⁰ =401.5 J/K

-252.6 kJ

-13.4 kJ

13.4 kJ

252.6 kJ

13.

For which of these processes is the value of ΔH expected to be negative?

1. The temperature increases when calcium chloride dissolves in water.

2. Steam condenses to liquid water

3. Water boils

4. Dry ice sublimates

1 and 2 only

3 and 4 only

2 and 3 only

1 only

14.

The equation that relates enthalpy, temperature and entropy is

Hess's Law

Second Law of Thermodynamics

Gibbs Free Energy

Calorimetry

15.

Solid magnesium dissolves in a solution of hydrochloric acid, releasing hydrogen gas and heat from a solution of magnesium chloride. What is the sign on ΔG for this reaction?

Negative because it is spontaneous

Negative because it is nonspontaneous

Positive because it is spontaneous

Positive because it is nonspontaneous

100 %

Enthalpy, Entropy, and Gibbs Free Energy

Total questions: 15

Worksheet time: 14mins

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