A75-kg copper block initially at 110°c is dropped into an insulated tank that contains 160 l of water at 15°c. determine the final equilibrium temperature and the total entropy change for this proces

T =43.61⁰C

ΔS = 0.84 KJ/K

Explanation:

Given that

Mass of copper block m₁ = 75 kg

Initial temperature of copper block ,T₁ = 110⁰C

Initial temperature of copper block ,water T₂ = 15⁰C

Specific heat for copper ,Cp₁=0.385 J/KkgK

Specific heat for water,Cp₂=4.187 KJ/kgK

Mass pf water ,m₂ = 0.16 x 1000 = 16 kg

Let's take final temperature = T

Heat lost by copper block = Heat gain by water

m₁ Cp₁ (T₁ - T) = m₂Cp₂(T-T₂)

T=316.61 K

T =43.61⁰C

The total change in entropy

ΔS = 0.84 KJ/K

an electric circuit