Question

$5.0g$ ice at $273K$ is added to $30g$ of water at $323K$ in a thermally insulated container. What is the final temperature?

• A. $289K$
• B. $608.43K$
• C. $152.43K$
• D. $-152.43K$

Answer 1

The correct option is A $289K$

Heat required to melt ice $=5\times 80=400cal$

Max. heat that can be lost by water $=30\times 1\times (323-273)=1500cal$

hence, heat left after melting the ice$=1100cal$
Heat lost $=$ Heat gained.

$\therefore$ $5\times 1\times (T-273)=1100+30\times 1(T-323)T=289K$