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Consider the reaction between graphite and oxygen gas to form carbon monoxide:

2C (s) graphite + O2 (g) → 2CO (g)    ΔHrxn = −221.0kJ

  1. Calculate the entropy change in the surroundings associated with this reaction occurring at 25 ∘C.
  2. Determine the sign of the entropy change for the system.
  3. Determine the sign of the entropy change for the universe.
  4. Is the reaction spontaneous?

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Robert Kubara
Robert KubaraLv10
4 Jan 2021

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Show transcribed image text

1. For each of the following statements, indicate whether it is true or false, and briefly explain your reasoning.

a) A spontaneous reaction always releases heat.

b) A spontaneous reaction is always a fast reaction.

c) The entropy of a system always increases for a spontaneous change.

d) The entropy of a system and its surroundings always increases for a spontaneous change.

e) The energy of a system always increases for a spontaneous change.

2. The reaction shown below is spontaneous at room temperature, but becomes nonspontaneous at a much higher temperature:

N2(g) + 3H2(g) --> 2 NH3(g)

From this fact alone, determine the signs of ΔH° and ΔS°, assuming that these do not change much with temperature. Explain your reasoning.

Can you please explain these in detail?

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