Question

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)

Answer 1

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.