The amount of heat energy required to convert 1 kg of ice at $- 10^{\circ} C$ to water at $100^{\circ} C$ is 7,77,000 J. Calculate the specific latent heat of ice.

Specific heat capacity of ice = 2100 J $k g^{- 1} K^{- 1}$ , specific heat capacity of water=4200 J k $g^{- 1} K^{- 1}$ .

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2 kg of ice melts when water at 100∘C is poured in a hole drilled in a block of ice. What mass of water was used? Given: specific heat capacity of water = 4200 Jkg−1K−1,specific latent heat of ice = 336×103Jkg−1

The correct option is C 1.6 kgHeat absorbed by ice =Q=2×336×103JNow this heat is provided by hot water Q=672×103=m×4200×(100−0)m=1.6 kg

$2 k g$ of ice melts when water at $100^{\circ} C$ is poured in a hole drilled in a block of ice. What mass of water was used?
Given: specific heat capacity of water = $4200 J k g^{- 1} K^{- 1}$ ,
specific latent heat of ice = $336 \times 10^{3} J k g^{- 1}$

The correct option is C $1.6 k g$
Heat absorbed by ice $= Q = 2 \times 336 \times 10^{3} J$
Now this heat is provided by hot water
$Q = 672 \times 10^{3} = m \times 4200 \times (100 - 0)$
$m = 1.6 k g$