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When a 11.9 gram sample of copper metal is dropped into a glass of cold water, the temperature of the copper drops from 55°C to 47°C. The specific heat capacity of copper is 0.39 J/g°C. How many Joules did the water absorb from the copper?
a- 55
b- 15.5
c- 9.7
d- 31.1

Respuesta :

Answer:

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Explanation:

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Eduard22sly

The amount of heat energy that will be absorbed by the water from the copper is 37.1 J

Data obtained from the question

  • Mass of copper = 11.9 g
  • Initial temperature (T₁) = 55 °C
  • Equilibrium temperature (Tₑ) = 47 °C
  • Specific heat capacity of copper (C) = 0.39 J/g°C
  • Heat absorbed by water =?

How to determine the heat

Heat lost by copper = heat gained by the water

Thus, we shall determine the heat lost by the copper in order to obtain the heat absorbed by the water

The heat lost by the copper can be obtained as follow:

  • Mass of copper (M) = 11.9 g
  • Initial temperature (T₁) = 55 °C
  • Equilibrium temperature (Tₑ) = 47 °C
  • Change in temperature (ΔT) = 55 – 47 = 8 °C
  • Specific heat capacity of copper (C) = 0.39 J/g°C
  • Heat (Q) =?

Q = MCΔT

Q = 11.9 × 0.39 × 8

Q = 37.1 J

Thus, the heat absorbed by the water is 37.1 J

Learn more about heat transfer:

https://brainly.com/question/6363778

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