Water of mass `m_(2) = 1 kg` is contained in a copper calorimeter of mass `m_(1) = 1 kg`. Their common temperature `t = 10^(@)C`. Now a piece of ice of mass `m_(2) = 2 kg` and temperature is `-11^(@)C` dropped into the calorimeter. Neglecting any heat loss, the final temperature of system is. [specific heat of copper `=0.1 Kcal//kg^(@)C`, specific heat of water `= 1 Kcal//kg^(@)C`, specific heat of ice `= 0.5 Kcal//kg^(@)C`, latent heat of fusion of ice `= 78.7 Kcal//kg`]

Options

A. `0^(@)C`
B. `4^(@)C`
C. `-4^(@)C`
D. `-2^(@)C`

Explanation

To solve the problem, we need to calculate the final temperature of the system after the ice is added to the water and copper calorimeter. We will use the principle of conservation of energy, where the heat lost by the water and the copper calorimeter will be equal to the heat gained by the ice.

### Step-by-step Solution:

1. **Identify the parameters:**
- Mass of water, \( m_2 = 1 \, \text{kg} \)
- Mass of copper calorimeter, \( m_1 = 1 \, \text{kg} \)
- Mass of ice, \( m_3 = 2 \, \text{kg} \)
...