Imagine the 10.0g of ice has an initial temperature of -5.0degreesC. Can someone calculate the energy needed to heat the ice, melt it, and heat the water to 54.5degreesC? (Cp of ice=2.108J/gdegreesC)

1 Answer
Mar 2, 2018

Total Energy required is: #5727.315J#

Explanation:

Latent Heat of Fusion of Ice: #334J/g# (#L#)

Formula: #E=mL#

Specific Heat Capacity of Ice: #2.108J/(g^oC)# (#c#)

Specific Heat Capacity of Water: #4.187J/(g^oC)# (#c#)

Formula: #E=mcT#

To calculate this, first we must find the energy required to raise the temperature of ice from #-5^oC# to it's melting point:

#E=mcT#

#E=10g * 5^oC * 2.108J/(g^oC)#

#E=105.4J#

Now, we must find the Energy required to convert the solid ice into liquid water at its melting point:

#E=mL#

#E=10g*334J/g#

#E=3340J#

Finally, we must find the Energy required to raise the temperature of water from #0^oC# to #54.5^oC#:

#E=mcT#

#E=10g * 54.5^oC * 4.187J/(g^oC)#

#E=2281.915J#

To calculate the total Energy needed, we need to add all the energy values up:

#105.4J+3340J+2281.915J#

#=5727.315J#

And there we have our answer.