The average molar heat capacities of ice and water are 37.8j/mol and 75.6j/ mol. The amount of heat required to change 10g of ice at -10 ^° c to water at 10^° c would be (a) 2376j (b)4752j (c) 3970j (d)1128j (e)1985

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Q. Calculate the quantity of heat required to convert 10 kg of ice at

0^{\circ}

to water at

50^{\circ} C

would be. Specific heat of water is 4200 J/kg

^{\circ} C

Q. Find the result of mixing

10 g

of ice at

- 10^{\circ} C

with

10 g

of water at

10^{\circ} C

. Specific heat capacity of ice =

2.1 J g^{- 1} K^{- 1}

, specific latent heat of ice =

336 J g^{- 1}

and specific heat capacity of water =

4.2 J g^{- 1} K^{- 1}

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 $g^{- 1} K^{- 1}$ .

Find the amount of heat in calories required to convert 10g of ice at –10°C to water at 10°C

[C of ice = 0.5 cal/g°C, C of water = 4.2J/g°C = 1 cal/g°C, L of ice = 80cal/g]

A 5 g piece of ice at $- 20^{\circ}$ C is put into 10 g of water at $30^{\circ}$ C. Assuming that heat is exchanged only between the ice and the water. Then find the heat required for phase change. Specific heat capacity of ice $= 2100 J k g^{- 1}^{\circ} C^{- 1}$ . Specific heat capacity of water $= 4200 J k g^{- 1}^{\circ} C^{- 1}$ and latent heat of fusion of ice $3.36 \times 10^{5} J k g^{- 1}$ .

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