Did I do this correct? If not, what is the correct way to solve it?

Question

An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calorimeter and water are in thermal equilibrium at 10.0°C. Two metallic blocks are placed into the water. One is a 75.0-g piece of copper at 60.0°C. The other has a mass of 70.0 g and is originally at a temperature of 100°C. The entire system stabilizes at a final temperature of 20.0°C.

I got 1822.143 J/(kg * deg C) is this value correct?

Answer 1

The aluminum and water gained heat:

Q = (mC_pΔT)_A + (mC_pΔT)_W

Q = (100)(0.890)(20 - 10) + (250)(4.186)(20 - 10) = 11355 joules

The metal lost the same amount of heat:

Q = (mC_pΔT)₁ + (mC_pΔT)₂

-11355 = (75)(0.385)(20 - 60) + (70)(x)(20 - 100)

-11355 = -1155 - 5600x

x = 1.82 j/g/°C

You are correct