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25 November, 12:47

If a 100.0 g sample of water at 60.0 c is added to a 100.0 g sample of water at 10.0 c determine the final temperature of water. Assume no heat is lost to the surroundings

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  1. 25 November, 16:16
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    We can use the heat equation,

    Q = mcΔT

    Where Q is the amount of energy transferred (J), m is the mass of the substance (kg), c is the specific heat (J g⁻¹ °C⁻¹) and ΔT is the temperature difference (°C).

    Let's say

    heat gained by 100.10 g of water at 10°C = Q₁

    heat lost from 100.0 g of water at 60 °C = Q₂

    Final temperature of the mixture = T

    Since, there is no heat is lost to the surroundings,

    Q ₁ = Q₂

    mc (T - 10) = mc (60 - T)

    Since, m is same for both sides (100.0 g) and c is a constant for the water, we can cut off m and c from both sides. Then,

    (T - 10) = (60 - T)

    2T = 60 + 10

    2T = 70

    T = 35 °C

    Hence, final temperature of water is T = 35 °C.
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