A 1.00-kg block of copper at 100°C is placed in an in- sulated calorimeter of negligible heat capacity containing 4.00 L of liquid water at 0.0°C. Find the entropy change of (a) the cop- per block, (b) the water, and (c) the universe.

the entropy change of the copper block = - 117.29 J/K

the entropy change of the water = 138.01 J/K

the entropy change of the universe = 20.72 J/K

Explanation:

For Copper block:

the mass of copper block = 1.00 kg

Temperature of block of copper = 100°C

= (100+273)K

= 373K

Standard Heat capacity for copper = 386 J/kg.K

For water:

We know our volume of liquid water to be = 4.00 L

At 0.0°C Density of liquid water  = 999.9 kg/m³

As such; we can determine the mass since :

∴ the mass of 4.00 L of liquid water at 0.0°C will be its density × volume.

= 999.9 kg/m³ ×

= 3.9996 kg

so, mass of liquid water = 3.9996 kg

Temperature of liquid water at 0.0°C = 273 K

Standard Heat Capacity of  liquid water = 4185.5 J/kg.K

Let's determine the equilibruium temperature between the copper and the liquid water. In order to do that; we have:

∴ the equilibrium temperature = 275.26 K

NOW, to determine the Entropy change of the copper block; we have:

The entropy change of the  water can also be calculated as:

The entropy change of the universe is the combination of both the entropy change of copper and water.