4.82 g of an unknown metal is heated to 115.0∘C and then placed in 35 mL of water at 28.7∘C, which then heats up to 34.5∘C. What is the specific heat of the metal?

The specific heat of metal is 2.34 J/g°C

Explanation:

To calculate the mass of water, we use the equation:

Density of water = 1 g/mL

Volume of water = 35 mL

Putting values in above equation, we get:

When metal is dipped in water, the amount of heat released by metal will be equal to the amount of heat absorbed by water.

The equation used to calculate heat released or absorbed follows:

     ......(1)

where,

q = heat absorbed or released

= mass of metal = 4.82 g

= mass of water = 35 g

= final temperature = 34.5°C

= initial temperature of metal = 115°C

= initial temperature of water = 28.7°C

= specific heat of metal = ?

= specific heat of water = 4.186 J/g°C

Putting values in equation 1, we get:

Hence, the specific heat of metal is 2.34 J/g°C

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