How much heat must be removed from 5.0g of water at 10°C to become ice at 0°C ? (my name is Kevin and I changed it to KPL cuz there is another kevin here)

How much heat must be remove from 5.0 g of water at 10 degrees celsius to become ice at 0 degree celsius

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To calculate the heat that must be removed, we need to use the specific heat capacity of water and the latent heat of fusion of ice. The specific heat capacity of water is 4.18 J/g°C, and the latent heat of fusion of ice is 334 J/g.

First, let's calculate the amount of heat that needs to be removed to bring the water from 10°C to 0°C using the specific heat capacity:

Q1 = m * c * ΔT1

Where:
Q1 = heat absorbed or released (in joules)
m = mass of the water (5.0g)
c = specific heat capacity of water (4.18 J/g°C)
ΔT1 = change in temperature (final temperature - initial temperature)

Q1 = 5.0g * 4.18 J/g°C * (0°C - 10°C)
Q1 = -209 J

Since we are going from a higher temperature to a lower temperature, the calculated value will be negative.

Now, let's calculate the amount of heat that needs to be removed for the water to freeze into ice at 0°C using the latent heat of fusion:

Q2 = m * L

Where:
Q2 = heat absorbed or released (in joules)
m = mass of the water (5.0g)
L = latent heat of fusion of ice (334 J/g)

Q2 = 5.0g * 334 J/g
Q2 = 1670 J

Now, to find the total amount of heat that needs to be removed, we sum up Q1 and Q2:

Q = Q1 + Q2
Q = -209 J + 1670 J
Q = 1461 J

Therefore, 1461 J of heat must be removed from 5.0g of water at 10°C to become ice at 0°C.

heat=5*1cal/gram*10C + 5*89 calories