If minimum possible work is done by a refrigenator in converting 100 grams of water at `0^@ C` to ice, how much heat (in calories) is released to the surroundings at temperature `27^@C` (latent heat of ice 80 Cal/gram) to the nearest integer ?

A refrigerator converts 100 g of water at 25^(@)C into ice at -10^(@)C in one hour and 50 minutes. The quantity of heat removed per minute is (specific heat of ice = 0.5 "cal"//g^(@)C , latent heat of fusion = 80 "cal"//g )

How many calories of heat will be required to convert 1 g of ice at 0^(@)C into steam at 100^(@)C

1 kg of ice at 0^(@)C is mixed with 1.5 kg of water at 45^(@)C [latent heat of fusion = 80 cal//gl. Then

50 g of ice at 0^@C is mixed with 50 g of water at 80^@C . The final temperature of the mixture is (latent heat of fusion of ice =80 cal //g , s_(w) = 1 cal //g ^@C)

m_(1) gram of ice at -10^(@)C and m_(2) gram of water at 50^(@)C are mixed in insulated container. If in equilibrium state we get only water at 0^(@)C then latent heat of ice is :

m_(1) gram of ice at -10^(@)C and m_(2) gram of water at 50^(@)C are mixed in insulated container. If in equilibrium state we get only water at 0^(@)C then latent heat of ice is :

An engine is working . It takes 100 calories of heat from source and leaves 80 calories of heat to sink . If the temperature of source is 127^(@) C, then temperature of sink is

10 g of ice at 0 C is slowly melted to water at 0 C. The latent heat of melting is 80 cal /g. the change in entropy is ?(cal/k)

Aluminium container of mass of 10 g contains 200 g of ice at -20^(@)C . Heat is added to the system at the rate of 100 calories per second. What is the temperature of the system after four minutes? Draw a rough sketch showing the variation of the temperature of the system as a function of time . Given: Specific heat of ice = 0.5"cal"g^(-1)(.^(@)C)^(-1) Specific heat of aluminium = 0.2"cal"g^(-1)(.^(@)C)^(-1) Latent heat of fusion of ice = 80"cal"g^(-1)

One gram of water at 100^(@)C is converted to steam at the same temperature. The amount of heat required is nearest to the value of