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 temperatu

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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 temperatu

re 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

Chemistry

1 answer:

Alik [6] · Answer 1 · 2023-09-16T06:56:55+03:00

The original temperature of the copper is 145.4 °C

<h3>What is temperature?</h3>

Temperature refers to the degree of hotness or coldness of a body. Now we know that the heat lost by the copper is equal to the heat gained by the water. The heat lost is negative while the heat gained is positive.

Hence;

-(mcdT)= mcdT

-(80.0 * 0.20 ( 26.9 - T)) = 100 * 4.12 * (26.9 - 22.3 )

-(430.4 - 16T) = 100 * 4.12 * (26.9 - 22.3 )

-430.4 + 16T = 1895.2

T = 1895.2 + 430.4 /16

T = 145.4 °C

The temperature of the copper is 145.4 °C.

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