Answer :
Final answer:
When ice at 0°C is mixed with water at 10°C, an energy exchange occurs where heat from the water melts some of the ice until equilibrium is achieved. This process results in a final temperature that is between 0°C and 10°C, depending on whether all the ice has melted and the water has started to warm up. However, the exact value cannot be one of the provided options since the final temperature would be 0°C if there is remaining unmelted ice.
Explanation:
Mixing Ice and Water to Determine Resultant Temperature
When 1 kg of ice at 0 degrees Celsius is mixed with 1 kg of water at 10 degrees Celsius, the final temperature can be determined by considering the energy exchanges during the melting of ice and the cooling of water until an equilibrium is reached. Since there are equal masses of ice and water, and both substances have a specific heat capacity (the amount of energy required to change the temperature of a substance), we can use this information to calculate the final temperature.
The specific heat capacity of water is 4.18 J/g°C, and the latent heat of fusion (the amount of heat required to turn ice into water without changing its temperature) is 334 J/g. The heat given up by the cooling of the warmer water can be used to melt some of the ice and raise the temperature of the resulting water until equilibrium is reached. The resultant temperature will be 0°C if all the ice has not melted, or a value between 0°C and 10°C if all the ice melts and the water starts to warm up.
Using the principle that energy lost by the warmer substance is equal to the energy gained by the colder substance (in this case, the ice melting and warming up), we can set up an equation that balances the energy exchanges. However, given the choices provided, a detailed heat energy balance calculation indicates that not all of the ice would have melted, therefore the final temperature would be 0°C, none of the options (a, b, c, d) are correct.
