A85.2 g copper bar was heated to 221.32 degrees celsius and placed in a coffee cup calorimeter containing 4250 ml of water at 22.55 degrees celsius. the final temperature of the water was recorded to be 26.15 degrees celsius. how much heat was lost by the copper

- 6402 J.

Explanation:

Q = m.C.ΔT, where,

Q is the amount of heat lost by the copper,

m is the mass of the copper (m = 85.2 g),

C is the specific heat of Cu (C = 0.385 J/g.°C),

ΔT is the temperature difference (the final temperature - the initial temperature (ΔT = 26.15 - 221.32 = - 195.17 °).

∴ The amount of heat lost by the copper Q = m.C.ΔT = ( 85.2 g) (0.385 J/g.°C) (- 195.17 °C) = - 6401.966 J ≅ - 6402 J.

the answer is option a.