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Energy and Entropy (Grade 10)

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Energy and Entropy

1. 
Which of the following describes a quantity that represents the amount of disorder or randomness in a system?
  1. energy
  2. enthalpy
  3. entropy
  4. potential energy
2. 
Which of the following situations represents an increase in entropy?
  1. A desk is cleaned up
  2. A room becomes messier over time
  3. Leaves on the ground are gathered into one pile
  4. Dirt is gathered into one pot
3. 
Which of the following represents a decrease in entropy?
  1. CO (l) [math]rarr[/math] CO (g)
  2. CO (s) [math]rarr[/math] CO (l)
  3. CO (g) [math]rarr[/math] CO (s)
  4. CO (s) [math]rarr[/math] CO (g)
4. 
Given the equation below:
HCl + energy [math]rarr[/math] H + Cl
How can this equation be described?
  1. This reaction is endothermic, and the heat is released
  2. This reaction is exothermic, and the heat is released
  3. This reaction is exothermic, and the heat is absorbed
  4. The reaction is endothermic, and the heat is absorbed
5. 
Which of the following phase changes is exothermic?
  1. condensation
  2. evaporation
  3. melting
  4. sublimation
6. 
Which of the following represents an exothermic process?
  1. The breaking of bonds in HCl
  2. Melting of ice cubes
  3. The formation of bonds in KCl
  4. Sublimation of carbon dioxide ice
7. 
Which of the following has the greatest entropy?
  1. CO (l)
  2. NO (g)
  3. CO (s)
  4. NO (s)
8. 
A person's hand heats up when his hand is placed on a solution of lithium bromide, as the lithium bromide is dissolved in water. Which statement correctly describes this process?
  1. The dissolving of lithium bromide is an endothermic process, and heat is absorbed.
  2. The dissolving of lithium bromide is an exothermic process, and heat is released.
  3. The dissolving of lithium bromide is a chemical change.
  4. The dissolving of lithium bromide is an endothermic process, and heat is released.
9. 
Explain how entropy changes during the dissolving of sodium hydroxide in water.



10. 
When carbon and oxygen combine to form carbon dioxide, ∆H=-393.5 kJ/mol. Classify this reaction as being endothermic or exothermic, and describe the reaction in terms of heat flow.



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