Answer:
Explanation:
δs sys = change in entropy of the system
= dQ / T
dQ is heat exchanged . It is negative as heat is given out and T = 273 k so
δs sys = - dQ / T
Its sign will be negative.
δs surr = dQ / T₁ , dQ is heat given by the water to freeze . It is positive
δs surr = + dQ / T₁ , T₁ is temperature of the surrounding
Sign of δs surr is positive .
δs univ = δs sys + δs surr
- dQ / T + dQ / T₁
T < T₁
dQ / T >dQ / T₁
- dQ / T + dQ / T₁ will be negative
δs univ will be negative .
The individual signs of ds univ, ds surr, and ds sys are given as follows
ds sys = change in entropy of the system
Generally, the equation for the ds sys is mathematically given as
ds sys = - dQ / T
Where dQ is heat exchanged
Hence, ds sys will be a negative sign
For ds surr
ds surr = dQ / T'
dQ=heat to freeze water
ds surr is positive
For ds univ
ds univ= ds sys + ds surr
ds univ= - dQ / T+ dQ / T'
ds univ is Negative
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