Kuster ~ K and E ~ Entropy

Which phase change represents a decrease in entropy?

• solid to liquid

• liquid to gas

• gas to liquid

• solid to gas

As carbon dioxide sublimes, its entropy

• decreases

• increases

• remains the same

Given the equation for the dissolving of sodium chloride in water:

Describe what happens to entropy during this dissolving process.

• entropy increases

• entropy decreases

• entropy is not affected by dissolving

Given the equation:

As H₂O(l) is added to KNO₃(s) to form KNO₃(aq),

the entropy of the system

• decreases

• increases

• remains the same

Even though the process is endothermic, snow can sublime. Which tendency in nature accounts for this phase change?

• a tendency toward greater entropy

• a tendency toward greater energy

• a tendency toward less entropy

• a tendency toward less energy

Which of these changes produces the greatest

increase in entropy?

• CaCO₃(s) → CaO(s) + CO₂(g)

• 2 Mg(s) + O₂(g) → 2 MgO(s)

• H₂O(g) → H₂O(l)

• CO₂(g) → CO₂(s)

Systems in nature tend to undergo changes toward

• lower energy and lower entropy

• lower energy and higher entropy

• higher energy and lower entropy

• higher energy and higher entropy

Given the balanced equation:

Which statement best describes this process?

• It is endothermic and entropy increases.

• It is endothermic and entropy decreases.

• It is exothermic and entropy increases.

• It is exothermic and entropy decreases.

At STP, a sample of which element has the highest entropy?

• Na(s)

• Br₂(l)

• Hg(l)

• F₂(g)

Given the balanced equation:

I₂(s) + energy → I₂(g)

As a sample of I₂(s) sublimes to I₂(g), the entropy of the sample

• increases because the particles are less

  randomly arranged

• increases because the particles are more

  randomly arranged

• decreases because the particles are less

  randomly arranged

• decreases because the particles are more

  randomly arranged