1. The problem statement, all variables and given/known data What will be the equilibrium temperature when a 245-g block of copper at 285° c is placed in a 145 g aluminium calorimeter cup containing 825 g of water at 12°c? 2. Relevant equations q=mcΔt qlost+qgained=0 -qlost=qgained -m1c1t1=m2c2t2 3. The attempt at a solution So this is what I did so far: Know : Copper Aluminium - 245 g= 0.245 kg - 145 g= 0.145 kg - specific heat capacity of copper = 0.385 j kg - ti=12°c - ti ( Inital temp)= 285°c -teq=? -teq=? Water -825 g=0.825 kg -ti=12°c -teq=? ( T equilibrium ) So I know qlost+ qgained= 0 then - qlost=qgained. In this case the qlost will be the copper. So this is what I used: ( Cu- copper; al-aluminium; & w- water) Mcu(Ccu)(Ticu-Teq)=Mal(Cal)(Teq-Ti) + Mw(Cw)(Teq-ti) (0.245 kg)(0.385)(285°c-Teq)=(0.145 kg)(9.2x10^2)(Teq-12°c)+(0.825kg)(4.18x10^3)(teq-12°c) Now when I come to this, I have no clue what to do : (0.094325)(285°c-Teq)=(133.4)(Teq-12°c)+(3448.5)(teq-12°c) Please let me know what I`m doing wrong, and how i can solve it completely.