Respuesta :
Answer:
a) and d) are false.
Explanation:
a) The second law of thermodynamics states that the entropy of the universe increases in a spon taneous  process and remains unchanged in an equilibrium process.
For a spontaneous process:
ΔSuniv = ΔSsys + ΔSsurr > 0
For a spontaneous process, the second law says that ΔSuniv must be greater than  zero, but it does not place a restriction on either ΔSsys or ΔSsurr. Thus, it is possible  for either ΔSsys or ΔSsurr to be negative, as long as the sum of these two quantities  is greater than zero.
d) A  reaction that does occur under the given set of conditions is called a spontaneous  reaction. We observe spontaneous physical and chemical processes every day,  including many of the following examples:
• A waterfall runs downhill, but never up, spontaneously.
• A lump of sugar spontaneously dissolves in a cup of coffee, but dissolved sugar  does not spontaneously reappear in its original form.
• Heat flows from a hotter object to a colder one, but the reverse never happens  spontaneously.
The statements that are false are:
a) If a chemical reaction is spontaneous then the Ssys must always be positive.
d) We don't need to worry about spontaneous reactions because they are rare.
Second law of thermodynamics:
It states that entropy of the universe increases in a spontaneous  process and remains unchanged in an equilibrium process.
For a spontaneous process:
ΔSuniv = ΔSsys + ΔSsurr > 0
For a spontaneous process, ΔSuniv must be greater than zero, but it does not place a restriction on either ΔSsys or ΔSsurr. Thus, it is possible  for either ΔSsys or ΔSsurr to be negative, as long as the sum of these two quantities  is greater than zero.
Also, spontaneous reactions  are rare.
Thus, options a and d are false statements.
Find more information about Second law of thermodynamics here:
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