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Complete combustion of a 0.350 g sample of a compound in a bomb calorimeter releases 14.0 kJ of heat. The bomb calorimeter has a mass of 1.20 kg and a specific heat of 3.55 J/(gi°C). If the initial temperature of the calorimeter is 22.5°C, what is its final temperature?

Respuesta :

The amount of heat released by the compound in a bomb calorimeter is 14.0kJ,
But heat released by the compound will be equal to the heat gained by the calorimeter. 
Heat energy = mass × specific heat × change in temperature.
Therefore;
14000 J = 1200 g × 3.55 ×(x-22.5)
14000 = 4260 (x-22.5)
x-22.5 = 3.286
        x = 25.786
           ≈ 25.9
Therefore, the final temperature is 25.8 °c
Eduard22sly

The final temperature of the calorimeter is 25.8 °C

From the question given above, the following data were obtained:

  • Mass (M) = 1.2 Kg = 1.2 × 1000 = 1200 g
  • Heat released (Q) = 14 KJ = 14 × 1000 = 14000 J
  • Initial temperature (T₁) = 22.5 °C
  • Specific heat capacity (C) = 3.55 J/gºC
  • Final temperature (T₂) =?

Q = MC(T₂ – T₁)

14000 = 1200 × 3.55(T₂ – 22.5)

14000 = 4260(T₂ – 22.5)

Clear bracket

14000 = 4260T₂ – 95850

Collect like terms

14000 + 95850 = 4260T₂

109850 = 4260T₂

Divide both side by 4260

T₂ = 109850 / 4260

T₂ = 25.8 °C

Learn more about heat transfer:

https://brainly.com/question/26061555

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