In an experiment on the specific heat of a metal a 0.20 kg block of the metal at `150^(@)`C is dropped in a copper calorimeter (of water equivalent 0.025 kg) containing 150 cc of water at `27^(@)`C. The final temperature is `40^(@)`C. Calcualte the specific heat of the metal. If heat losses to the surroundings are not negligible, is our answer greater or smaller than the actual value of specific heat of the metal?

Options

A. 0.02
B. 0.2
C. 0.01
D. 0.1

Explanation

To solve the problem of finding the specific heat of the metal, we will follow these steps:

### Step 1: Identify the given data
- Mass of the metal block, \( m_m = 0.20 \, \text{kg} = 200 \, \text{g} \)
- Initial temperature of the metal, \( T_{m_i} = 150 \, ^\circ C \)
- Mass of water, \( m_w = 150 \, \text{cc} = 150 \, \text{g} \) (since the density of water is \( 1 \, \text{g/cm}^3 \))
- Water equivalent of the calorimeter, \( W_c = 0.025 \, \text{kg} = 25 \, \text{g} \)
- Initial temperature of water, \( T_{w_i} = 27 \, ^\circ C \)
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