Calculate the amount of heat required to completely sublime 57.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublim

Question

Calculate the amount of heat required to completely sublime 57.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.

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Thu Nguyệt 3 years 2021-08-31T03:51:23+00:00 2 Answers 36 views 0

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  1. niczorrrr
    0
    2021-08-31T03:52:46+00:00
    Reply

    Answer:

    41.48KJ

    Explanation:

    the amount of heat(q)=nΔH_{sub}

    n represents the number of moles of the substance

    n=\frac{mass of CO_{2} }{Molar mass of CO_{2} }

    mass of carbondioxide = 57g

    the molar mass of carbondioxide is obtained by adding the atomic mass of the individual elements present

    atomic mass of carbon = 12g

    atomic mass for oxygen = 16 × 2 =32g

    Molar mass of carbondioxide =  12 + 32 = 44g/mole

    ∴ n = 57÷44

    n = 1.2955moles

    ΔH_{sub} represents the heat of sublimation for the substance in that sublimation process = 32.3kJ/mol

    the amount of heat (q) = 1.2955 × 32.3

    q= 41.84KJ

    the amount of heat required to completely sublime 57g of carbondioxide is 41.48KJ

  2. Nick
    0
    2021-08-31T03:52:57+00:00
    Reply

    Answer:

    41.83 J.

    Explanation:

    The amount of heat required to completely sublime CO₂ is

    Q = cm’ ……………… Equation 1

    Where Q = Amount of heat required to sublime CO₂, c = heat of sublimation of CO₂, m’ = number of moles of CO₂.

    Molar mass of CO₂ = 12 + (16×2) = 12×32 = 44 g/mole,

    If 1 mole of CO₂ contains a mass of 44 g,

    57/44 moles of CO₂ will contain a mass of 57 g.

    1.295 moles.

    Given: c = 32.3 kJ/mol, n = 1.295 mol.

    Substitute into equation 1

    Q = 32.3(1.295)

    Q = 41.83 J.

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