Calculate the amount of energy in joules that must be added to 245.0 g of ice at -45.0 ºC to

turn it all into liquid water at 0.00 ºC.  Hint, two separate calculations must be done and then

added together.

To calculate the energy required to convert 245.0 g of ice at \(-45.0\ ^\circ\text{C}\) to liquid water at \(0.00\ ^\circ\text{C}\), we need to break the problem into two parts:

1. **Heating the ice** from \(-45.0\ ^\circ\text{C}\) to \(0.0\ ^\circ\text{C}\).
2. **Melting the ice** at \(0.0\ ^\circ\text{C}\) to turn it into liquid water.

### Step 1: Heating the ice

To calculate the heat required to raise the temperature of ice from \(-45.0\ ^\circ\text{C}\) to \(0.0\ ^\circ\text{C}\

Calculate the amount of energy in joules that must be added to 245.0 g of ice at -45.0 ºC to turn it all into liquid water at 0.00 ºC. Hint, two separate calculations must be done and then added together.

Learn how to calculate the total energy required to heat 245.0 g of ice from -45.0 ºC to 0.00 ºC and melt it into water. This solution involves heat transfer calculations using specific heat capacity and latent heat, and applies concepts from thermodynamics. Suitable for high school students in Grades 11-12.

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