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27 September, 06:01

125 g of dry ice (solid CO2) is dropped into a beaker containing 500 g of 66°C water. The dry ice converts directly to gas, leaving the solution.

When the dry ice is gone, the final temperature of the water is 29°C.

What is the heat of vaporization of solid CO2? (cwater = 1.00 cal/g⋅°C)

a. 37 cal/gb. 74 cal/gc. 111 cal/gd. 148 cal/g

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  1. 27 September, 06:07
    0
    The right option is (d).148 cal/g

    Explanation:

    Specific Latent Heat Of Vaporization: This is the quantity of heat required to change unit mass of a substance from either liquid to vapor, or solid to vapor without a change in temperature.

    Heat gained by dry ice = Heat lost by the water

    Q₁ = Q₂ ... equation 1

    Where Q₁ = heat gained by the dry ice, Q₂ = heat lost by the water.

    Q₁ = lm₁ ... equation 2

    Q₂ = cm₂ΔT ... equation 3

    Substituting the equation 1 into Equation 2,

    lm₁ = cm₂ΔT ... equation 4

    Where l = heat of vaporization of the dry ice, m₁ = mass of the dry ice, c = specific heat capacity of water, m₂ = mass of water, ΔT = change in temperature = T₁ - T₂

    Making l the subject of formula in equation 4

    l = cm₂ΔT/m₁ ... equation 5

    Where c = 1.00 cal/g.°C, m₂ = 500g, ΔT = T₁ - T₂ = 66-29 = 37°C, m₁ = 125 g.

    Substituting these values into equation 5

    ∴ l = (1 * 500 * 37) / 125

    l = 148 cal/g

    The right option is (d).148 cal/g
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