The final temperature of the copper and water in the calorimeter given the data is 30.3 °C
<h3>Data obtained from the question</h3>
- Specific heat capacity of copper (C꜀) = 0.385 J/gºC
- Mass of copper (M꜀) = 95 g
- Temperature of copper (T꜀) = 77.9 °C
- Mass of water (Mᵥᵥ) = 42 mL = 1 × 42 = 42 g
- Temperature of water (Tᵥᵥ) = 20.4 °C
- Specific heat capacity of the water (Cᵥᵥ) = 4.184 J/gºC
- Equilibrium temperature (Tₑ) =?
<h3>How to determine the equilibrium temperature </h3>
Heat loss = Heat gain
MᵥᵥC(Tᵥᵥ – Tₑ) = M꜀C(Tₑ – M꜀)
95 × 0.385 (77.9 – Tₑ) = 42 × 4.184(Tₑ – 20.4)
36.575(77.9 – Tₑ) = 175.728(Tₑ – 20.4)
Clear bracket
2849.1925 – 36.575Tₑ = 175.728Tₑ – 3584.8512
Collect like terms
2849.1925 + 3584.8512 = 175.728Tₑ + 36.575Tₑ
6434.0437 = 212.303Tₑ
Divide both side by 212.303
Tₑ = 6434.0437 / 212.303
Tₑ = 30.3 °C
Learn more about heat transfer:
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