Question

8630 kJ of heat is added to 2.84 kg ice initially at -5.00°C. What is the final temperature of the resulting water (whatever state it may be in)?

Answer 1

Heat added to ice is Q= 8630kJ

Lets first see the amount of heat needed to bring ice to 0 degree celsius temperature.

Now we know that Heat capacity of ice is

then heat needed to lowering the temperature of ice is

then using all given and known values,

Now heat require for conversion of ice to water is

where L= Latent Heat of fusion= 334 kJ/kg

then we'll have

Since   

Thus whole amount of the ice will be converted into water.

then remaining heat energy is

  

Now Specific heat capacity of water,

then heat energy needed to raise temperature of water to 100 degree celsius,

  

  

Again thus added heat will raise the temperature of water to 100 degree celsius.

Now remaining energy will be

  

Now energy needed to convert it to steam,

where L= Latent Heat of vaporization= 2264.76 kJ/kg

then we'll have

Again since thus it will be converted into steam.

Now if the final temperature is T, then we'll have

  

where Specific heat capacity of steam,

Using all calculated, given and known values in above,

(ANS)