Question

How much energy will be released if 200 gr of water at 30°C is converted into ice at O°C?​

Answer 1

Answer:

The latent heat required to melt all of the ice to liquid water at 0 C is 10 x 80 cal. The heat lost by the water starting at 10 C and reducing to zero degrees Celsius is 10 x 10 cal.

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Answer 2

Answer:

The energy will be released for conversion of 200 g of water at 30°C into ice at 0°C will be 67.2 KJ.

Explanation:

We know that specific heat capacity of water $= 4.2KJkg ^{-1}deg^{-1}$

Change in temperature ΔT$= T_{1}-T_{2} =30-0=30^{o}C$

mass of water $= 200g$

Heat released = m.S.ΔT

Energy released $=(200)(4.2)(30)=67.2KJ$

Therefore the energy releases in the given phase transition is equal to 67.2KJ.