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Thermodynamics Review

An educational illustration showing thermodynamic concepts, like heat transfer, reactions, and phase changes, with diagrams and symbols related to thermodynamics.

Thermodynamics Challenge Quiz

Test your knowledge of thermodynamics with our engaging quiz! This quiz covers essential concepts such as exothermic and endothermic reactions, entropy changes, and phase transitions. Whether you're a student or a teacher, this quiz can help reinforce key thermal principles in a fun and interactive way.

The quiz consists of multiple-choice questions, calculations, and open-ended questions to ensure a comprehensive assessment of your understanding. Get ready to dive into the world of thermodynamics!

8 Questions2 MinutesCreated by ExcitedElectron42

Which of the examples below are examples of exothermic reactions?

Water freezing into ice

Lighting a match

The reaction inside a cold pack

The combustion of natural gas

For exothermic reactions like the ones in question 1, what does q_system equal?

Qsys > 0

Qsys < 0

In an endothermic reaction, energy is _____ and the sign of ΔH is ________

Absorbed, positive

Absorbed, negative

Released, negative

Released, positive

2C(s) + H₂(g) ---> C₂H₂(g)

ΔH° = ??? kJ

Calculate the enthalpy for this reaction knowing the ΔH values for these three other reaction.

C₂H₂(g) + ⁵⁄₂O₂(g) → 2CO₂(g) + H₂O(l)	ΔH° = −1299.5 kJ
C(s) + O₂(g) → CO₂(g)	ΔH° = −393.5 kJ
H₂(g) + ¹⁄₂O₂(g) → H₂O(l)	ΔH° = −285.8 kJ

In this reaction: CaCO_3(s) → CaO_(s) + CO_{2(g) ,}

is the entropy (ΔS) increasing or decreasing?

Increasing

Decreasing

In the phase change diagram, why does the temperature not change in two spots on the graph while heat is still added?

The material is undergoing a phase changes

The material stopped absorbing heat

The environment is at a new temperature

We ran out of fuel

The heat added is being used to break/form bonds and does not change the temperature

In setting up an experiment, you have 500 ml of water in a beaker sitting at room temperature (25°C). You also have a 100 g copper ball that you have been heating over a bunsen burner to 100°C. You then decide to drop the ball into the beaker of water and record the change in temperature. If given enough time to come to equilibrium, what will the final temperature in the beaker be?

Specfici heat capacities: Water, 4.184 (J/g°•C) Copper, 0.385 (J/g°•C)

True or False: A reaction with a positive ΔH and a negative ΔS will be spontaneous at all temperatures

True

False

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