Question

1. A 0.400 kg sample of aluminum (c=9.10 x10^2hj/kg•C) at 95°C is dropped into a 0.550 kg pot of water, which is at 18°C. What temperature will the mixture come to ? 2. How much thermal energy is absorbed by a 0.0220 kg ice cube as it melts? For this problem let the latent heat of fusion in water be 3.4×10^5 j/Kg.

Answer 1

1. To find the final temperature of the mixture, we can use the principle of conservation of energy. The heat lost by the aluminum will be equal to the heat gained by the water. We can use the equation:

(mass of aluminum * specific heat capacity of aluminum * change in temperature of aluminum) = (mass of water * specific heat capacity of water * change in temperature of water)

Plugging in the values, we get:

(0.400 kg * 9.10 x 10^2 J/kg·°C * (final temperature - 95°C)) = (0.550 kg * 4.18 x 10^3 J/kg·°C * (final temperature - 18°C))

Solving this equation will give us the final temperature of the mixture.

2. To find the thermal energy absorbed by the ice cube as it melts, we can use the equation:

thermal energy = mass of ice cube * latent heat of fusion

Plugging in the values, we get:

thermal energy = 0.0220 kg * 3.4 x 10^5 J/kg

Solving this equation will give us the amount of thermal energy absorbed by the ice cube.

Let me know if you need any further assistance or if there's anything else I can help you with!