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In-s [12.5K]
3 years ago
5

Calculate the change in entropy of 3 moles of liquid water if you heat it from 5˚C to 95˚C. The molar heat capacity of liquid wa

ter is 75.38 J/molK. Please report your answer one point past the decimal with the unit J/K.
Chemistry
1 answer:
IceJOKER [234]3 years ago
4 0

<u>Answer:</u> The entropy change of the liquid water is 63.4 J/K

<u>Explanation:</u>

To calculate the entropy change for same phase at different temperature, we use the equation:

\Delta S=n\times C_{p}\times \ln (\frac{T_2}{T_1})

where,

\Delta S = Entropy change

C_{p} = molar heat capacity of liquid water = 75.38 J/mol.K

n = number of moles of liquid water = 3 moles

T_2 = final temperature = 95^oC=[95+273]K=368K

T_1 = initial temperature = 5^oC=[5+273]K=278K

Putting values in above equation, we get:

\Delta S=3mol\times 75.38J/mol.K\times \ln (\frac{368}{278})\\\\\Delta S=63.4J/K

Hence, the entropy change of the liquid water is 63.4 J/K

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