A 2.45 g sample of a substance suspected of being pure gold is warmed to 72.9 ∘C and submerged into 15.6 g of water initially at 24.2 ∘C. The final temperature of the mixture is 26.6 ∘C.

Question

A 2.45 g sample of a substance suspected of being pure gold is warmed to 72.9 ∘C and submerged into 15.6 g of water initially at 24.2 ∘C. The final temperature of the mixture is 26.6 ∘C.
Part A
What is the specific heat capacity of the unknown substance?
Express your answer using two significant figures.

DrBob222 · Accepted Answer

[mass metal x specific heat metal x (Tfinal - Tinitial)] + [mass H2O x specific heat H2O x (Tfinal - Tinitial)] = 0
[2.45 g x specific heat metal x (26.6 - 72.9)] + [15.6 g x4.184 J/g*C x [26.6 - 24.2)] = 0
Solve for specific heat metal. Post your work if you get stuck.