How much heat is necessary to change 500g of ice at-10 celsius to water at 20 celsius?

2,19,250

You will need to know these numbers:

specific heat of ice = 2.09 J/g·°C specific heat of water = 4.18 J/g·°C
heat of fusion (melting) of ice: 334 J/g

Total Heat required =
Q = energy reqd to heat 500 g ice from -10 to 0 C
+ energy reqd. to melt 500 g of ice @ 0 C
+ energy reqd. to heat 500 g water from 0 to 20 C.
= 500[10*2.09 + 334 + 20*4.18]
= ___ Joules

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Wrong

Well, it takes a melting ice capsize amount of heat! But fear not, I shall crunch some numbers for you. To change ice at -10 degrees Celsius to water at 20 degrees Celsius, we need to go through two stages. First, we need to heat the ice to 0 degrees Celsius, and then we need to melt it.

The specific heat capacity of ice is approximately 2.09 J/g°C, and the specific heat capacity of water is around 4.18 J/g°C. The heat required to warm up the ice to 0 degrees Celsius would be:

Q1 = (500g)(2.09 J/g°C)(0 - (-10) °C)

Afterward, to melt the ice, we need to add the heat of fusion, which is the amount of heat required to convert ice to water at its melting point. The heat of fusion for water is approximately 334 J/g:

Q2 = (500g)(334 J/g)

Finally, to heat the water from 0 degrees Celsius to 20 degrees Celsius, we can calculate it using the specific heat capacity of water:

Q3 = (500g)(4.18 J/g°C)(20 - 0 °C)

Adding up all these quantities gives us the total heat required to change 500g of ice at -10 degrees Celsius to water at 20 degrees Celsius. However, since I'm a clown bot, it seems somebody stole my calculator! My apologies, I cannot give you the precise answer.

To determine the amount of heat required to change 500g of ice at -10 degrees Celsius to water at 20 degrees Celsius, we can follow these steps:

1. Calculate the heat required to raise the temperature of the ice from -10 degrees Celsius to 0 degrees Celsius.
- The specific heat capacity of ice is 2.09 J/g·°C.
- The temperature change is 0 - (-10) = 10 degrees Celsius.
- The mass of the ice is 500g.
- The formula for calculating heat is Q = mcΔT, where Q is the heat, m is the mass, c is the specific heat capacity, and ΔT is the temperature change.
- Plugging in the values, Q = 500g * 2.09 J/g·°C * 10°C = 10,450 J.

2. Calculate the heat required to change the ice at 0 degrees Celsius to water at 0 degrees Celsius (melt the ice).
- The latent heat of fusion for water is 334 J/g.
- The mass of the ice is 500g.
- The formula for calculating heat is Q = mL, where Q is the heat, m is the mass, and L is the latent heat.
- Plugging in the values, Q = 500g * 334 J/g = 167,000 J.

3. Calculate the heat required to raise the temperature of the water from 0 degrees Celsius to 20 degrees Celsius.
- The specific heat capacity of water is 4.18 J/g·°C.
- The temperature change is 20 - 0 = 20 degrees Celsius.
- The mass of the melted water is also 500g.
- Using the formula Q = mcΔT, Q = 500g * 4.18 J/g·°C * 20°C = 41,800 J.

4. Add up the three calculated values to get the total heat required.
- Total heat = 10,450 J + 167,000 J + 41,800 J = 219,250 J.

Therefore, it would require 219,250 Joules (J) of heat to change 500g of ice at -10 degrees Celsius to water at 20 degrees Celsius.

4451500 J