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30 May, 19:01

A sample of wood has a heat of combustion of 3.29 kJ/g. What quantity of the wood must be burned to heat 250. g of water from 18°C to 85°C? Once again, the specific heat capacity of water is 4.18 J/°C·g.

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  1. 30 May, 19:28
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    The quantity of wood that must be burned = 21.28 g

    Explanation:

    Heat produce by the wood = heat absorbed by the water

    Q₁ = Q₂ ... Equation 1

    Where Q₁ and Q₂ are heat produce by the wood and heat absorbed by the water respectively.

    Q₁ = c₁m₁ ... Equation 2

    Q₂ = c₂m₂ (T₂-T₁) ... Equation 3

    Substituting equation 2 and 3 into equation 1

    c₁m₁ = c₂m₂ (T₂-T₁) ... Equation 4

    making m₁ the subject of the equation,

    m₁ = c₂m₂ (T₂-T₁) / c₁ ... Equation 5

    Where c₁ = heat of combustion of the wood, c₂ = specific heat capacity of water, m₁ = mass of the wood, m₂ = mass of water, T₁ = initial temperature, T₂ = final Temperature.

    Given: c₁ = 3.29 kJ/g = 3290 J/g, c₂ = 4.18 J/g.°C, m₂ = 250 g, T₂ = 85 °C, T₁ = 18 °C

    Substituting these values into equation 4,

    m₂ = 4.18*250 (85-18) / 3290

    m₂ = 70015/3290

    m₂ = 21.28 g

    Thus the quantity of wood that must be burned = 21.28 g
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