$($b$)$ A container containing $1000$ kg of liquid

water initially at $\frac{80}{\frac{?}{?}}$ deg C is brought into a

room. The

$4m5m7m$ room is well insulated and

sealed, and initially at a temperature of $220$ C

Answer the following:

$($i$)$ What is the final temperature of the water

and the total amount of energy

transferred from the water to the air?

$($ii$)$ What is the entropy change of the water?

$($iii$)$ Despite the entropy change of the water

being calculated as negative in Part $($ii$)$

of this question, show that this does not

violate the Increase in Entropy Principle.

$($Note: In your solution, you can assume the

specific heat of water is constant at $4\mathrm{.}18k\frac{J}{?}$

kgK $)$