How much energy is required to heat 36.9g of ice at 0 degrees celsius to water at 0 degrees celsius?
q = mass ice x heat fusion.
To calculate the amount of energy required to heat ice at 0 degrees Celsius to water at 0 degrees Celsius, we need to consider the three steps involved:
1. Heating the ice from -10°C to 0°C.
2. Melting the ice at 0°C.
3. Heating the water from 0°C to 0°C.
Now, let's calculate each step separately:
Step 1: Heating the ice from -10°C to 0°C.
The specific heat capacity of ice is 2.09 J/g°C. This means that it takes 2.09 Joules of energy to raise the temperature of 1 gram of ice by 1 degree Celsius.
The temperature change for this step is 0°C - (-10°C) = 10°C.
The mass of the ice is given as 36.9 grams.
Using the formula: Energy = mass x specific heat capacity x temperature change,
we can calculate the energy required to raise the temperature of the ice:
Energy = 36.9 g x 2.09 J/g°C x 10°C
Step 2: Melting the ice at 0°C.
The heat of fusion (also known as the latent heat of fusion) for ice is 334 J/g. The heat of fusion represents the energy required to change a substance from a solid to a liquid at its melting point (0°C for ice).
Using the formula: Energy = mass x heat of fusion,
we can calculate the energy required to melt the ice:
Energy = 36.9 g x 334 J/g
Step 3: Heating the water from 0°C to 0°C.
The specific heat capacity of water is 4.18 J/g°C.
Using the formula: Energy = mass x specific heat capacity x temperature change,
we can calculate the energy required to raise the temperature of the water:
Energy = 36.9 g x 4.18 J/g°C x 0°C
Finally, to find the total energy required, we sum up the energies from each step:
Total energy = Energy in Step 1 + Energy in Step 2 + Energy in Step 3
Now you can plug in the numbers and calculate the total energy required.