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Units of Heat

How much heat...

Question

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

4200 J

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2100 J

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1050 J

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525 J

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Solution

The correct option is C $2100 J$
Heat released= $m L + m c (T_{1} - T_{2}) = 5 \times 336 + 5 \times 4.2 \times 20$
Heat released = $2100 J$

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Similar questions

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.

100 g

- 10^{o} C

100^{o} C

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

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

= 336 J g^{- 1}

100 g

20^{o} C

10^{o} C

73.5 m i n

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

336 J g^{- 1}

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

10 g

- 10^{o} C

10 g

10^{o} C

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

= 336 J g^{- 1}

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

2 K g

0^{0} C

20^{0} C

3, 34, 000 J / K g

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

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