Answer:
a) and d) are false.
Explanation:
a) The second law of thermodynamics states that t<u>he entropy of the universe increases in a spon
taneous process and remains unchanged in an equilibrium process.</u>
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) <u>A reaction that does occur under the given set of conditions is called a</u> 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.
Answer:
Truth
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<span>(3) Atomic masses are a weighted average of the naturally occurring isotopes.
</span>
Here, we found this answer my looking at the key words 'naturally occurring isotopes'
An isotope is a different amount of neutrons, making the atomic mass change.
Each particle has two possibilities: either it is on the left hand side or it is on the right hand side.
The probability of having them equally split is
P(100,100) = 200C100 / 2^200
where 200C100 is the binomial coefficient.
For the uneven distribution we have
P= 2 * 200C160 / 2^200
where the factor 2 comes in because we could have 160/40 or 40/160 as a division.
So the ratio of probabilities is
200C100 /(2 * 200C160 )
= 2.2 * 10^16
Hope this helps!
