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Thermodynamics ...

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  • Question 1
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    Based on the first law of thermodynamics, which one of the following is correct ?

  • Question 2
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    The Born Haber cycle below represents the energy changes occurring at 298K when KH is formed from its elements :
    v : $${ \Delta H }_{ atomisation }$$ K = 90 kJ/mol
    w : $${ \Delta H }_{ ionisation }$$ K = 418 kJ/mol
    x : $${ \Delta H }_{ dissociation }$$ H = 436 kJ/mol
    y : $${ \Delta H }_{ electron affinity }$$ H = 78 kJ/mol
    z : $${ \Delta H }_{ lattice }$$ KH = 710 kJ/mol
    In terms of the letters v to z the expression for
    (i) $$\Delta $$H for the reaction
    $$2K$$(s) + $${ H }_{ 2 }$$(g) $$\longrightarrow $$ $$2KH$$(s).
    will be $$\Delta $$$$H =_____?

  • Question 3
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    The Born Haber cycle below represents the energy changes occurring at 298K when $$KH$$ is formed from its elements
    v : $${ \Delta H }_{ atomisation }$$ $$K = 90 kJ/mol$$
    w : $${ \Delta H }_{ ionisation }$$ $$K = 418 kJ/mol$$
    x : $${ \Delta H }_{ dissociation }$$ $$H = 436 kJ/mol$$
    y : $${ \Delta H }_{ electron affinity }$$ $$H = 78 kJ/mol$$
    z : $${ \Delta H }_{ lattice }$$ $$KH = 710 kJ/mol$$
    On complete reaction with water, $$0.1 g$$ of $$KH$$ gave a solution requiring 25 $${ cm }^{ 3 }$$ of 0.1M $$HCl$$ for neutralisation.Calculate the relative atomic mass of potassium from this information.

  • Question 4
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    Directions For Questions

    The Born Haber cycle below represents the energy changes occurring at 298K when $$KH$$ is formed from its elements :
    v : $${ \Delta H }_{ atomisation }$$ $$K = 90 kJ/mol$$
    w : $${ \Delta H }_{ ionisation }$$ $$K = 418 kJ/mol$$
    x : $${ \Delta H }_{ dissociation }$$ $$H = 436 kJ/mol$$
    y : $${ \Delta H }_{ electron affinity }$$ $$H = 78 kJ/mol$$
    z : $${ \Delta H }_{ lattice }$$ $$KH = 710 kJ/mol$$

    ...view full instructions

    Write a balanced equation for the reaction of $$KH$$ with water.

  • Question 5
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    The amount of heat required to raise the temperature of a substance through 1$$^o$$C is called

  • Question 6
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    Specific heat capacity of lead is $$120\space J\space kg^{-1}\space K^{-1}$$. When $$7200J$$ of heat is supplied to $$5kg$$ of lead, the rise in temperature is

  • Question 7
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    $$H_2C=\! = CH_2(g)+ H_2 (g)\longrightarrow  H_3C -\!\! \! - CH_3(g)$$
    $$The

    \: bond \: energy \: of \: C -\!\! \! -H, \:C -\!\! \! -C, \:C=\! =C

    \:and \:H-\!\! \! -H \: are \: 414, \: 347,615 \: and \: 435 \: kJ \:

    mol^{-1} \: respectively.$$
    If the enthalpy change of the above reaction is $$x$$ $$kJ$$, then $$-x$$ is

  • Question 8
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    The $$\Delta H_{f}^{0}$$ for $$CO_{2} (g), CO(g)$$ and $$H_{2}O(g)$$ are $$-393.5, -110.5$$ and $$-241.8\ kJ\ mol^{-1}$$ respectively. The standard enthalpy change (in kJ) for the reaction
    $$CO_{2} (g) + H_{2}(g) \rightarrow CO(g) + H_{2}O(g)$$ is

  • Question 9
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    Hess's law is used to calculate

  • Question 10
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    For the equilibrium $$H_{2}O(l) \rightleftharpoons H_{2}O(g)$$ at $$1\ atm$$ and $$298\ K$$

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