Question

1. When we add heat to ice at -10. deg C, what first happens, and then if we continue to add more heat what else happens?

2. When the ice is heated to the melting point, and more heat is added, what happens to the temperature?

3. Once the ice is all melted, as we add more heat, what happens to the temperature? And this continues until what happens?

4. How many calories are required if 25.0 g of ice is heated from -10.0 deg C to 85.0 dec C?

Answer 1

Q1.

first happens --> heat will eventually incrase its tempearture up to 0°C as ice, if we keep adding heat to ice, we will have a mix of water and ice at 0°C, if we keep adding heat, then eventually we get water at 0°C

Q2

As stated before:

if we keep adding heat to ice, we will have a mix of water and ice at 0°C, if we keep adding heat, then eventually we get water at 0°C

Q3

IF we metl all ice to water, at 0°C, then we will increase water's temperature up to 100°C max as water

Q4.

Fin Q for m = 25 g of ice from -10°C to 85°C

Q1 = -10° to 0

Q2 = 0-0 latent heat

Q3 0 to 85

Cp ice = 2.01 J/g°C ; Cp water = 4.184 J/g°C;

LH ice = 334 kJ/kg;

Q1 = (25)(2.01)(0--10) = 502.5

Q2 = 25*334 = 8350

Q3 = (25*4.184)(85-0) = 8891

Qtotal =502.5 + 8350 + 8891 = 17743.5J = 17.743 kJ