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45 g of water at 50^@C in a beaker is co...

45 g of water at `50^@`C in a beaker is cooled when 50 g of copper at `18^@`C is added to it. The contents are stirred till a final constant temperature is reached. Calculate the final temperature. The specific heat capacity of copper is 0.39 J `g^(-1)K^(-1)` and that of water is 4.2 J `g^(-1) K^(-1)`. State the assumption used.

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To solve the problem, we will apply the principle of calorimetry, which states that the heat lost by the hotter substance (copper) will be equal to the heat gained by the cooler substance (water). ### Step-by-Step Solution: 1. **Identify Given Data:** - Mass of water, \( m_w = 45 \, \text{g} \) - Initial temperature of water, \( T_{i,w} = 50^\circ C \) - Specific heat capacity of water, \( S_w = 4.2 \, \text{J/g} \cdot \text{K} \) ...
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