A 1 kg block of ice, at 0.0 celcius is added to a picnic cooler. How much heat will the ice remove as it melts into water at 0.0celcius?

To calculate the amount of heat the ice will remove as it melts into water, you can use the specific heat formula. The specific heat of ice is 2.09 J/g°C, and the heat required to melt ice is known as heat of fusion, which is 334 J/g.

First, convert the mass of the ice from kilograms to grams:
1 kg = 1000 g

Next, calculate the heat required to raise the temperature of the ice from 0.0°C to 0.0°C:
Q1 = mass × specific heat × change in temperature
= 1000 g × 2.09 J/g°C × (0.0°C - 0.0°C)
= 0 J

Since the temperature remains constant during the phase change from ice to water, no heat is required to raise the temperature to the melting point.

Finally, calculate the heat required to melt the ice into water:
Q2 = mass × heat of fusion
= 1000 g × 334 J/g
= 334,000 J

Therefore, the ice will remove 334,000 J of heat as it melts into water at 0.0°C.

First, note the correct spelling of celsius.

q removed = 1000 g x heat fusion.