How much heat energy is released when 5.0 g of water at $20^{0} C$ changes to ice at $0^{0} C$ ? Take specific heat capacity of water equal to 4.2 $J g^{- 1} C^{- 1}$ , specific latent heat of fusion of ice = 336 $J g^{- 1}$ .

Open in App

Solution

Mass of water m = 5.0 g
specific heat capacity of water c = $4.2 J g^{- 1} K^{- 1}$ specific latent heat of fusion of iceL = $336 J g^{- 1}$
Amount of heat energy released when 5.0 g of water at $20^{o} C$ changes into water at $0^{o} C$ = 5 x 4.2 × 20 = 420 J.
Amount of heat energy released when 5.0g of water at $0^{o} C$ changes into ice at $0^{o} C$ = 5 × 336J = 1680 J.
Total amount of heat released = 1680 J + 420 J = 2100 J.

Suggest Corrections

Similar questions

Q. Find the result of mixing

10 g

of ice at

- 10^{o} C

with

10 g

of water at

10^{o} 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}

10 g of ice at 0 $^{\circ} C$ absorbs 5460 J of heat energy to melt and change t water at 50 $^{\circ} C$ . Calculate the specific latent heat of fusion of ice. (Specific heat capacity of water is 4200 J $K g^{- 1} K^{- 1}$ .

Q. How much energy is required to change

2 K g

of ice at

0^{0} C

into water at

20^{0} C

? (specific latent of heat of fusion of water =

3, 34, 000 J / K g

, specific heat capacity of water =

4200 J {K g}^{- 1} K^{- 1}

Q. A thermos-flask of negligible heat capacity contains 100 g of ice. Calculate the amount of water in the flask after condensation.

(Given that: Latent heat of ice

= 336 J g^{- 1}

, latent heat of steam

= 2260 J g^{- 1}

, specific heat capacity of water

= 4.2 J g^{- 1} C^{- 1}

)

Calculate the amount of heat released when 5.0 g of water at 20 °C is changed into ice at 0 °C.

Specific heat capacity of water = 4.2J g^-1 °C^-1, Specific latent heat of fusion of ice = 336 J g^-1.

Join BYJU'S Learning Program

How much heat energy is released when 5.0 g of water at 200C changes to ice at 00C? Take specific heat capacity of water equal to 4.2 Jg−1C−1, specific latent heat of fusion of ice = 336 Jg−1.

How much heat energy is released when 5.0 g of water at $20^{0} C$ changes to ice at $0^{0} C$ ? Take specific heat capacity of water equal to 4.2 $J g^{- 1} C^{- 1}$ , specific latent heat of fusion of ice = 336 $J g^{- 1}$ .