The value of specific heat for copper is 390 J/kg⋅°C, for aluminun is 900 J/kg⋅°C, and for water is 4186 J/kg⋅°C. What will be the equilibrium temperature when a 265 g block of copper at 235°C is placed in a 135g aluminum calorimeter cup containing 865 g of water at 14.0°C? Express your answer using three significant figures.

the equilibrium temperature Te = 19.9°C

Explanation:

Given;

specific heat for copper Cc is 390 J/kg⋅°C

for aluminun Ca is 900 J/kg⋅°C,

for water Cw is 4186 J/kg⋅°C

Mass of copper Mc= 265 g = 0.265kg

Temperature of copper Tc = 235°C

Mass of aluminium Ma = 135g = 0.135 kg

Temperature of aluminium Ta = 14.0°C

Mass of water Mw= 865 g = 0.865kg

Temperature of water Tw = 14.0°C

The equilibrium temperature can be derived by;

Te = (MaCaTa + McCcTc + MwCwTw)/(MaCa + McCc+ MwTw)

Substituting the values;

Te = ( 0.135×900×14 + 0.265×390×235 + 0.865×4186×14)/(0.135×900 + 0.265×390 + 0.865×4186)

Te = 19.939°C

Te = 19.9°C

i think the answer would be reserve.