**Question:**

**The specific heat of water $=4200 \mathrm{~J} \mathrm{~kg}^{-1} \mathrm{~K}^{-1}$ and the latent heat of ice $=3.4 \times 10^{5} \mathrm{~J} \mathrm{~kg}^{-1} .100$ grams of ice at $0^{\circ} \mathrm{C}$ is placed in $200 \mathrm{~g}$ of water at $25^{\circ} \mathrm{C}$. The amount of ice that will melt as the temperature of water reaches $0^{\circ} \mathrm{C}$ is close to (in grams):**

$61.7$

$63.8$

$69.3$

$64.6$

Question of from chapter.

JEE Main Previous Year Sep. 04, 2020 (I)

Correct Option: 1

**Solution:**

### Related Questions

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