Find the final equilibrium temperature when 10.0 g of milk at 10. c is added to 1.60 x 10^2g of coffee with a temperature of 90.0c assume the specific hw=eats of coffee and milk are the same as for water

Question

Chemistry

Santiago Bryant

4 September, 13:12

Find the final equilibrium temperature when 10.0 g of milk at 10. c is added to 1.60 x 10^2g of coffee with a temperature of 90.0c assume the specific hw=eats of coffee and milk are the same as for water

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Answers (1)

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Noelle Ellis · Answer 1

The concept that can be used in order to answer this item is that of the conservation of heat among the system. We let T be equal to the final temperature. The equation that would allow us to relate the initial and final conditions of both substances is as follows,

m₁cp₁ (T - T₁) = m₂cp₂ (T₂ - T)

The first entity, 1, is the milk and the second entity, 2, is the coffee. We are given that the specific heats of both substances are just equal so we can eliminate them from the equation. Substituting the known values,

(10 g) (T - 10°) = (1.60 x 10^2 g) (90° - T)

The value of T from the equation is 85.29°C.

Answer: 85.29°C