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    Heat Capacity, Enthalpy, IM Forces and Radius of Pt Atom

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    1.Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20 C to convert it to liquid water at 60.0 C. Given: Specific heat (ice)=2.1 J/goC Specific heat(water)=4.18 J/goC H (fus)=6.0 kJ/mol
    420 J
    2,900 J
    6,300 J
    63 kJ
    7.5 J

    2. The major enthalpy of Boron tribromide (BBr3) is 30.5 kJ/mol, and its normal boiling point is 91oC. What is the vapor pressure of BBr3 at 20oC?
    11.5 torr
    311 torr
    5.31 torr
    143 torr
    66.1 torr

    3. Each of the following substances is a liquid at -50oC. Place these liquids in order of increasing vapor pressure: Dimethyl ether (CH3OCH3), propane (C3H8), ethanol (CH3CH2OH).
    Ethanol<propane<dimethyl ether
    Ethanol<dimethyl ether<propane
    Propane<dimethyl ether<ethanol
    Dimethyl ether<ethanol<propane
    Propane<ethanol<dimethyl ether

    4. Platinum (Pt) has a face centered cubic crystal structure and a density of 21.5 g/cm3. What is the radius of the platinum atom(pm:picometer).
    69 pm
    98 pm
    139 pm
    196 pm
    277 pm

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    https://brainmass.com/chemistry/energetics-and-thermodynamics/heat-capacity-enthalpy-forces-radius-atom-376891

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    1.Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20oC to convert it to liquid water at 60.0oC. Given: Specific heat (ice)=2.1 J/goC Specific heat(water)=4.18 J/goC H (fus)=6.0 kJ/mol
    420 J
    2,900 J
    6,300 J
    63 kJ
    7.5 J

    This is a problem that needs to be done in three steps:
    1. Find heat required to bring ice from -20.0 deg to 0 deg.
    2. Find heat required to melt ice.
    3. Find heat require to bring ice from 0 deg to 60.0 deg.

    1. Find heat required to bring ice from -20.0 deg to 0 deg.
    m = mass of ice
    c = specific heat of ice
    delta T = change in temp (0 - -20.0 = 20.0 deg)
    q = mc delta T = 10.0 g x 2.1 J/g/deg C x 20.0 deg = 420 J

    2. Find heat required to melt ice.
    kJ must be converted to J, because all of the answers are in J. 18.02 g/mol is the molar mass of water.
    q = delta H (fus) x moles = 6.0 kJ/mol x 1000 J/kJ x (10.0 g/18.02 g/mol) = 3330 J

    3. Find heat require to bring ice from 0 deg to 60.0 deg.
    m = mass of water
    c = specific heat of water
    delta T = change in temp (60.0 -0 = 60.0 deg)
    q = mc delta T = 10.0 g x 4.18 J/g/deg C x 60.0 deg = 2508 J
    Add them all together, and account for sig ...

    Solution Summary

    Questions regarding heat capacity, enthalpy, intermolecular forces and finding the radius of a platinum atom are answered in detail with full explanations and working.

    $2.49

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