Question

When 50.0 g of water at 95.0°C is transferred to 35.0 g of water at 28.0°C, what is the final temperature of the mixture of water?

A) 61.5°C
B) 76.0°C
C) 71.5°C
D) 52.5°C

Answer 1

The final temperature of the mixture of water is C) 71.5°C.. By equating the heat lost and gained by the two samples of water, the final temperature of 71.5°C is obtained, indicating the point of equilibrium between the two masses of water.

Explanation.

When calculating the final temperature of the water mixture, the formula for heat transfer,
`\(Q = mcΔT\),` where \(Q\) is the heat transferred, \(m\) is the mass
`, \(c\)` is the specific heat capacity, and
`\(ΔT\) i`s the change in temperature, is utilized. By applying this formula and accounting for the heat lost and gained by each sample of water, the final temperature is determined to be 71.5°C.

This calculation involves equating the heat lost by the hotter water to the heat gained by the cooler water until they reach thermal equilibrium, resulting in the final temperature. The process involves the conservation of energy, where the heat lost by the hotter water is equal to the heat gained by the cooler water until both reach the same final temperature. The specific heat capacity of water (4.18 J/g°C) is considered in the calculation to accurately determine the final temperature.

This calculation demonstrates the principles of heat transfer and the conservation of energy in reaching thermal equilibrium between two substances at different temperatures. By equating the heat lost and gained by the two samples of water, the final temperature of 71.5°C is obtained, indicating the point of equilibrium between the two masses of water.