Answered

Welcome to Westonci.ca, the place where your questions find answers from a community of knowledgeable experts. Get the answers you need quickly and accurately from a dedicated community of experts on our Q&A platform. Join our platform to connect with experts ready to provide precise answers to your questions in different areas.

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

#SPJ5

Thanks for using our platform. We aim to provide accurate and up-to-date answers to all your queries. Come back soon. We hope this was helpful. Please come back whenever you need more information or answers to your queries. Keep exploring Westonci.ca for more insightful answers to your questions. We're here to help.