Question

Suppose that during the Melting Ice lab, 65,000 J of energy were transferred to 450 g of water at 20˚C. What would have been the final temperature of the water?

Answer 1

To find the final temperature of the water, we can use the principle of energy conservation. We can calculate the heat gained by the water and the heat required to melt the ice. By setting the total heat gained equal to the heat lost by the hot water, we can solve for the final temperature.

Step-by-step explanation:

To find the final temperature of the water, we can use the principle of energy conservation, which states that the heat lost by the hot water is equal to the heat gained by the cold water. First, we need to determine the heat gained by the water:

1. Calculate the heat required to raise the temperature of the water from 20˚C to its final temperature (let's call it ). We can use the formula Q = mcΔT, where Q is the heat, m is the mass of the water, c is the specific heat of water, and ΔT is the temperature change.
2. Next, calculate the heat required to melt the ice. Since we know the energy transferred (65,000 J) and the mass of water (450 g), we can use the formula Q = mL, where Q is the heat, m is the mass of water, and L is the latent heat of fusion for water (which is 334 J/g).

Now that we have the total heat gained by the water and the ice, we can set it equal to the heat lost by the hot water and solve for. Once we have we will have the final temperature of the water.