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Homework #1

  • Page ID
    42480
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    Due on Tuesday, Jan 19, 2016.

    Q1

    Calculate the final temperature that results from:

    1. 2.48 g sample of Nickel at an initial temperature of 16.7 °C that absorbs 59 J of heat (Note: \(C_p\) of Ni is 0.440 J/g°C)
    2. 72.8 g of water at an initial temperature of 72.5°C that releases 270 J of heat (Note: \(C_{p}\) (water)=4.184 J/g°C)

    Q4

    When 1.36 g of sucrose (\(C_{12}H_{22}O_{11}(s)\)) is burned in a bomb calorimeter, the temperature increases by 6.6 °C. If the heat capacity of the calorimeter is 3.40 kJ/°C, what must be the internal energy change (\(\Delta U\)) for the combustion of one mole of sucrose, in kJ/mol?

    Q65

    The heat of combustion of 2-butanol at 298 K is -35.7 kJ/g (which was determined by a bomb calorimeter). Determine the internal energy change \(∆U\) and enthalpy change \(∆H\) for the combustion of one mole of 2-butanol at 298 K.

    Q69

    Use Hess’s Law to determine the standard enthalpy of reaction for the following reaction:

    \[3C_{(Graphite)} + 4H_{2(g)} \rightarrow C_3H_{8(g)}\]

    by using the information below.

    1. \(C_3H_{8(g)} + 5O_{2(g)} \rightarrow 3CO_{2(g)} + 4H_2O_{(l)} \;\;\Delta H^\circ = -4567.1kJ\)
    2. \(C_{(graphite)} + O_{2(g)} \rightarrow CO2(g) \;\;\Delta H^\circ = -432.5kJ\)
    3. \(H_{2(g)} + 1/2O_{2(g)} \rightarrow H_2O_{(l)} \;\;\ \Delta H^\circ = -123.4kJ\)

    Q87

    Calculate the standard enthalpy of reaction for the following reaction:

    \[C_6H_{6(l)} +\frac{15}{2} O_{2 (g)} \rightarrow 6 CO_{2 (g)} + 3 H_2O_{(l)}\]

    Given these values:

    • \(\Delta H^\circ_f = +49.0\; kJ/mol\) for \(C_6H_{6(l)}\)
    • \(\Delta H^\circ_f = -393.5\; kJ/mol\) for \(CO_{2(g)}\)
    • \(\Delta H^\circ_f = -285.8\; kJ/mol\) for \(H_2O_{(l)}\)

    Homework #1 is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts.

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