A block of copper, of unkown mass, initially at 75.7 celcius is immersed in a beaker...

A block of copper, of unkown mass, initially at 75.7 celcius is immersed in a beaker containing 125.5 g of water at 20.7 celcius. At thermal equilibrium, the final temperature is 24.2 celcius. What is the mass of the copper if the specific heat capacities of water is 4.18 J/(gC) and copper is 0.385 J/(gC))

Expert Solution

Heat gained by water = m*s*delta T

= 125.5 g * 4.18 J/(gc) *(24.2-20.7)

= 1383.6 J

Heat lost by copper = m*s*delta T

= m*0.385 ?/(gC) *(75.7-24.2) C

= m*19.83 J

At thermal equilibrium

heat gained by water = heat lost by copper

1383.6 J = m*19.83 J

m = 1383.6J/19.83 J

= 69.8 g

Mass of copper = 69.8 g

queen_honey_blossom answered 4 hours ago

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