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A 95.0 g sample of copper (Cp = 0.20 J/°C·g) is heated to 82.4°C and then placed in a container of water (Cp= 4.18 J/°C·g) at 22.0°C. The final temperature of the water and the copper is 25.1°C. What was the mass of the water in the original container? Assume that all heat lost by the copper is gained by the water.

Sagot :

sanstale12226

(C:) 84.0 g H2 O

Its the right answer

mahima6824soni

The mass of the water in the original container by assuming that all heat lost by the copper is gained by the water is 116.23 g.

What is mass?

Mass is the term that told the quantity of a matter.

Given the mass of copper = 110g

The specific heat capacity of copper is 0.20 j/C g

The initial temperature of  copper is 82.4 C

The final temperature of copper and water is 24.9 C

Now, we would determine the mass of the water.

From the formula for sensible heat, ΔH = m × c × ΔT

Where, H = sensed heat,

m = mass,

ΔT = temperature change

Putting the above values in the equation.

ΔH = m × c × ΔT

110 × 0.20 × ( 82.4 - 24.9 ) = mw × 4.186 × (24.9 - 22.3)

1265 J = mw × 10.8836 or mw = 116.23 g

Thus,  the mass of water is 116.23 g.

To learn more about mass, refer to the link:

https://brainly.com/question/8475948

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