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28 February, 14:34

How much heat (kJ) is absorbed by 229.1 g of water in order for the temperature to increase from 25.00∘C to 32.50∘C?

Q2) Calculate the amount of heat required to raise the temperature of a 34 g sample of water from 9 ∘C to 23 ∘C.

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  1. 28 February, 17:28
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    (Q1) 9.42 kJ.

    (Q2) 1.999 kJ

    Explanation:

    Heat: This is a form of Energy that brings about the sensation of warmth.

    The S. I unit of Heat is Joules (J).

    The heat of a body depend on the mass of the body, specific heat capacity, and temperature difference. as shown below

    Q = cm (t₂-t₁) ... Equation 1

    (Q1)

    Q = cm (t₂-t₁)

    Where Q = amount of heat absorbed, c = specific heat capacity of water, m = mass of water, t₁ = initial temperature, t₂ = final temperature.

    Given: m = 229.1 g = 0.2991 kg, t₁ = 25.0 °C, 32.50 °C

    Constant: c = 4200 J/kg.°C

    Substituting into equation 1

    Q = 0.2991*4200 (32.5-25)

    Q = 1256.22 (7.5)

    Q = 9421.65 J

    Q = 9.42 kJ.

    Hence the heat absorbed = 9.42 kJ

    (Q2)

    Q = cm (t₂-t₁)

    Where Q = amount of heat required, c = specific heat capacity of water, m = mass of water, t₁ = initial temperature, t₂ = final temperature.

    Given: m = 34 g = 0.034 kg, t₁ = 9 °C, t₂ = 23 °C

    Constant: c = 4200 J/kg.°C

    Q = 0.034*4200 (23-9)

    Q = 142.8 (14)

    Q = 1999.2 J

    Q = 1.999 kJ.

    Thus the Heat required = 1.999 kJ
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