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A 80.0 g sample of copper (specific heat = 0.20 J/g °C ) is heated and then added to 100 g water at 22.3 °C. The final temperature of the water and copper is 26.9°C. What is the original temperature of the copper sample, assuming that all the heat lost by the copper is gained by the water?

Respuesta :

samueladesida43

The original temperature of the copper sample, assuming that all the heat lost by the copper is gained by the water is 147.08°C.

How to calculate temperature?

The temperature in a calorimetry experiment can be calculated using the following formula:

Q = mc∆T

Where;

  • Q = quantity of heat absorbed or released
  • m = mass of substance
  • c = specific heat capacity
  • ∆T = change in temperature

For a calorimetry;

Q(water) = -Q(metal)

mc∆T (water) = -(mc∆T) (metal)

100 × 4.18 × 4.6 = - (80 × 0.20 × {26.9 - x}

1922.8 = -430.4 + 16x

16x = 2353.2

x = 147.08°C

Therefore, the original temperature of the copper sample, assuming that all the heat lost by the copper is gained by the water is 147.08°C.

Learn more about temperature at: https://brainly.com/question/11464844

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