A silver block, initially at 59.8 ∘C, is submerged into 100.0 g of water at 24.6 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.6 ∘C.

Question

A silver block, initially at 59.8 ∘C, is submerged into 100.0 g of water at 24.6 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.6 ∘C.
What is the mass of the silver block?

R_scott · Answer

heat lost by silver = heat gained by water heat change = mass * specific heat * temperature change

Doc48 · Answer

Σq = q(Ag) + q(H₂O) = (mcΔT)Ag + (mcΔT)H₂O = 0
=> m(Ag)(0.240j/g∙ᵒC)(26.6-59.8)ᵒC + (100g)(4.184(0.240j/g∙ᵒC)(26.6-24.6)ᵒC = 0
=> m(Ag)(-7.968j/g) + (836.8j) = 0
=> m(Ag) = (836.8/7.968)g = 105.2g