You will have to provide a bit more information. How much ice are we talking about? Does the heat source provide 300 W?Firben said:1. How much heat ΔQ is consumed to raise the ice temperature from Ti = -20 Celsius to meltingpoint Tf = 0 ? how long does it take ?
2. dQ/dt = H = 300 W
dQ = cmΔT
3 I got it to be 2.49 * 10^-21 J. Is it right ?
The formula for calculating the heat consumed to raise the ice temperature is ΔQ = m * c * ΔT, where m is the mass of the ice, c is the specific heat capacity of ice, and ΔT is the change in temperature.
The specific heat capacity of ice is 2.09 J/g°C. This value can be found in most physics or chemistry textbooks or by conducting experiments.
No, the heat consumed to raise the ice temperature is not the same as the heat released when the ice melts. The heat consumed is used to increase the temperature of the ice, while the heat released is the energy needed for the ice to change from a solid to a liquid state.
Yes, the amount of heat consumed to raise the ice temperature does depend on the initial temperature of the ice. It takes more energy to raise the temperature of ice that is closer to its melting point than ice that is at a lower temperature.
In a real-life scenario, you would need to know the mass of the ice, the specific heat capacity of ice, and the change in temperature. You would then use the formula ΔQ = m * c * ΔT to calculate the heat consumed. It's important to note that this calculation may not be exact as there are other factors, such as heat loss to the environment, that can affect the final temperature of the ice.