A heated copper block at `130^(@)C` loses 340 J of heat to the surroundings which are at room temperature of `32^(@)C` . Calculate
(i) the entropy change of the system ( copper block ) (ii) the entropy change in the surrounding
(iii) the total entropy change in the universe due to this process
Assume that the temperature of the block and the surroundings remains constant.

Explanation

To solve the problem, we will calculate the entropy changes step by step.

### Given Data:
- Temperature of the copper block, \( T_{block} = 130^\circ C = 130 + 273.15 = 403.15 \, K \)
- Temperature of the surroundings, \( T_{surroundings} = 32^\circ C = 32 + 273.15 = 305.15 \, K \)
- Heat lost by the copper block, \( Q = 340 \, J \)

### Step 1: Calculate the Entropy Change of the System (Copper Block)
...