<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:

where,
= Entropy change
= molar heat capacity of liquid water = 75.38 J/mol.K
n = number of moles of liquid water = 3 moles
= final temperature = ![95^oC=[95+273]K=368K](https://tex.z-dn.net/?f=95%5EoC%3D%5B95%2B273%5DK%3D368K)
= initial temperature = ![5^oC=[5+273]K=278K](https://tex.z-dn.net/?f=5%5EoC%3D%5B5%2B273%5DK%3D278K)
Putting values in above equation, we get:

Hence, the entropy change of the liquid water is 63.4 J/K
1. Aqeuous or dissolved
2.AgNO3+ NaCl are reactants
3. NaNO3 is precipitate
4. Reaction is endothermic(Delta stands for Heat)
5. Neither a reactant nor a product, MnO2 is a catalyst
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