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.