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Born-haber cycle - class-XI

born-haber cycle

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Questions

Question 1 Multiple Choice (Single Answer)

Which of the following can be calculated from Born-Haber cycle for $Al _2O _3$?

  1. Lattice energy of $Al _2O _3$
  2. Electron affinity of O-atom
  3. Ionisation energy of Al
  4. All of these
Question 2 Multiple Choice (Single Answer)

In the series $Sc(Z=21)$ to $Zn(Z=30)$, the enthalpy of atomisation of which element is least?

  1. Sc
  2. Mn
  3. Cu
  4. Zn
Question 3 Multiple Choice (Single Answer)

The lattice energy of CsI(s) is −604 KJ/mol, and the enthalpy of solution is 33 KJ/mol. How would you calculate the enthalpy of hydration (KJ) of 0.65 moles of CSI? Enter a numeric answer only, do not include units in your answer?

  1. $738 KJ $
  2. $ 10 KJ $
  3. $-371 kj$
  4. $-822 KJ$
Question 4 Multiple Choice (Single Answer)

Consider the following reaction,
$2A + B \rightarrow C + 2D$, $\Delta H _{1} = 10$
$A + 2C \rightarrow 2D + B$, $\Delta H _{2} = -5$ What is $\Delta H$ of reaction $A + 2B \rightarrow 3C$?

  1. $-5$
  2. $+5$
  3. $+10$
  4. $+15$
Question 5 Multiple Choice (Single Answer)

Determine ${ \Delta  }{ U }^{ o }$ at $300K$ for the following reaction using the listed enthalpies of reaction:


$4CO(g)+8{ H } _{ 2 }(g)\longrightarrow 3{ CH } _{ 4 }(g)+{ CO } _{ 2 }(g)+2{ H } _{ 2 }O(l)$

$C _{(graphite)}+1/2{ O } _{ 2 }(g)\longrightarrow CO(g);\quad \Delta { { H } _{ 1 } }^{ o }=-110.5kJ$

$CO(g)+1/2{ O } _{ 2 }(g)\longrightarrow { CO } _{ 2 }(g);\quad \Delta { { H } _{ 2 } }^{ o }=-282.9kJ$

${ H } _{ 2 }(g)+1/2{ O } _{ 2 }(g)\longrightarrow { H } _{ 2 }O(l);\quad \Delta { { H } _{ 3 } }^{ o }=-285.8kJ$

$C _{(graphite)}+2{ H } _{ 2 }(g)\longrightarrow { CH } _{ 4 }(g);\quad \Delta { { H } _{ 4 } }^{ o }=-74.8kJ$

  1. $653.5\ kJ$
  2. $-686.2\ kJ$
  3. $-747.4\ kJ$
  4. None of these
Question 6 Multiple Choice (Single Answer)

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
${ \Delta H } _{ i }$ of K is ${ \Delta H } _{ i }$ = $w/2$.
If true enter 1, else enter 0.

  1. 0
  2. 1
  3. 2
  4. 3
Question 7 Multiple Choice (Single Answer)
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.
  1. $39$
  2. $40$
  3. $41$
  4. None of these
Question 8 Multiple Choice (Single Answer)

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 : ${ \Delta H } _{ lattice }$ $KH = 710 kJ/mol$

Calculate the value of $\Delta $$H$ showing all your working.

  1. 124 kJ/mol
  2. -124 kJ/mol
  3. 124 J/mol
  4. None of these
Question 9 Multiple Choice (Single Answer)

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
${ \Delta H } _{ electron affinity }$ of H is ${ \Delta H } _{ electron affinity }$  is __.
I

  1. $y$
  2. $y/2$
  3. $2y$
  4. $y/3$
Question 10 Multiple Choice (Single Answer)

The energy change for the alternating reaction that yields chlorine sodium $(Cl^{+}Na^{-})$ will be:

$2Na(s)\, +\, Cl _2(g)\,\rightarrow\, 2Cl^{+}Na^{-}(s)$

Given that:

Lattice energy of $NaCl\,=\,-787\, kJ\,mol^{-1}$

Electron affinity of $Na\,=\,-52.9\, kJ\, mol^{-1}$

Ionisation energy of $Cl\, =\, +\,1251\, kJ\, mol^{-1}$

BE of $Cl _2\,=\,244\, kJ\, mol^{-1}$

Heat of sublimation of $Na(s)\, =\,107.3\, kJ\, mol^{-1}$

$\Delta H _f(NaCl)\, =\,-411\, kJ\, mol^{-1}$.

  1. +640 kJ
  2. +1280 kJ
  3. -410 kJ
  4. +410 kJ
Question 11 Multiple Choice (Single Answer)

The lattice energy of NaCl(s) using the following data will be:

heat of sublimation of $Na(s)\,=\,S$

$(IE) _1$ of $Na\,(g)\,=\,I$

bond dissociation energy of $Cl _2\,(g)\,=\,D$

electron affinity of $Cl\,(g)\,=\,-E$

heat of formation of $NaCl(s)\,=\,-Q$
  1. Lattice energy $-U\, =\, S\, +\, I\, +\,\displaystyle \frac{D}{2}\, -\, E\, -\,Q$
  2. Lattice energy $-U\, =\, S\, -\, I\, +\,\displaystyle \frac{D}{2}\, -\, E\, -\,Q$
  3. Lattice energy $-U\, =\, S\, +\, I\, +\,\displaystyle \frac{D}{2}\, +\, E\, -\,Q$
  4. Lattice energy $-U\, =\, S\, -\, I\, -\,\displaystyle \frac{D}{2}\, +\, E\, +\,Q$
Question 12 Multiple Choice (Single Answer)

Use the following data to calculate second electron ainity of oxygen, i.e., for the process
$O^{-}(g) + e^{-}(g)  \rightarrow O^{2-}(g)$
Is the $O^{2-}$ ion stable in the gas phase?.Why is it stable in solid MgO?
Heat of sublimation of $Mg(s) = + 147.7 kJ mol^{-1}$
Ionisation energy of Mg(g) to form
$Mg^{2+}(g) = + 2189.0 kJ mol^{-1}$
Bond dissociation energy for $O _2 = + 498.4 kJmol^{-1}$
First electron affinity of $O(g) = - 141.0 kJ mol^{-1}$
Heat formation of $MgO(s) = -601.7 kJ mol^{-1}$
Lattice energy of $MgO = -3791.0 kJ mol^{-1}$

  1. 601.7
  2. 744.4
  3. 1346.1
  4. 147.7
Question 13 Multiple Choice (Single Answer)

Select correct statement.

  1. Both lattice energy and hydration energies decrease with ionic size.
  2. Lattice energy can be calculated using Born-Haber cycle.
  3. If the anion is larger compared to the cation, the lattice energy will remain almost constant within a particular group.
  4. All the above are correct statements.
Question 14 Multiple Choice (Single Answer)

Caesium chloride is formed according to the following equation:

$Cs(s)+0.5{Cl} _{2}(g)\longrightarrow CsCl(s)$

The enthalpy of sublimation of $Cs$, enthalpy of dissociation of chlorine, ionization energy of $Cs$ and electron affinity of chlorine are $81.2, 243.0, 375.7$ and $-348.3kJ$ ${ol}^{-1}$. The energy change involved in the formation of $CsCl$ is $388.6\ kJ.{mol}^{-1}$. Calculate the lattice energy of $CsCl$.

  1. $-618.7\ kJ{mol}^{-1}$
  2. $+618.7\ kJ{mol}^{-1}$
  3. $1315.2\ kJ{mol}^{-1}$
  4. None of these
Question 15 Multiple Choice (Single Answer)

The ionization potential of ithium is 520 KJ/ mole .The energy required to convert 70 mg of lithum atoms in gaseous state into $Li^{+}$ ions is ______________.

  1. 52 KJ
  2. 5.2 KJ
  3. 520 KJ
  4. 52 J
Question 16 Multiple Choice (Single Answer)

The atoms of hydrogen combine to form a molecule of hydrogen gas, the energy of the $H _2$ molecule is:

  1. Greater than that of seperate atoms
  2. Equal to that of seperate atoms
  3. Lower than that of seperate atoms
  4. Some times lower and some times higher
Question 17 Multiple Choice (Single Answer)

Which of the following bonds has the highest bond energy?

  1. Si-Si
  2. Si=Si
  3. Si-O
  4. Si=O
Question 18 Multiple Choice (Single Answer)

Born Haber cycle is used to determine:

  1. electron affinity
  2. lattice energy
  3. crystal energy
  4. all the above
Question 19 Multiple Choice (Single Answer)

Choose the correct statement about the process (I) and (II).


$\displaystyle Na^{+} _{(g)}\xrightarrow{(I)}Na _{\left ( g \right )} \xrightarrow {(II)}Na _{\left ( s \right )}$

  1. In $(I)$ energy released. $(II)$ energy absorbed
  2. In both $(I)$ and $(II)$ energy is absorbed
  3. In both $(I)$ and $(II)$ energy is released
  4. In $(I)$ energy absorbed, $(II)$ energy released
Question 20 Multiple Choice (Single Answer)

For the maximum ionic character during bond formation ,_________ on cation and a __________ anion are required.

  1. low charge, high charge
  2. low charge, low charge
  3. high charge , no charge
  4. none of these
Question 21 Multiple Choice (Single Answer)

The standard formation reaction for aluminium oxide is $4Al(s) + 6O(g)\rightarrow 2Al _2O _3(s)$. This statement is false because:

  1. aluminium is not in its standard state
  2. the reaction should be written for one mole of Al
  3. The reaction is prevented by a thin film of $Al _2O _3$ formed on the surface of Al
  4. none of these
Question 22 Multiple Choice (Single Answer)

Standard enthalpy of formation $(\Delta H _f)$ of which of the following is zero at $25^0C$ ?

  1. White phosphorous
  2. Red phosphorous
  3. Red lead $(Pb _3O _4)$
  4. $H^+(g)$
Question 23 Multiple Choice (Single Answer)

The heat change for the reaction: $C(s) + S(s)\rightarrow CS _2(l)$, known as:

  1. heat of transition
  2. heat of fusion
  3. heat of vapourisation
  4. heat of formation
Question 24 Multiple Choice (Single Answer)

Enthalpy of a solution of $ CsBr(s)$ is $10\ kJ/mol$.If the enthalpies of hydration of $Cs^+(g)$ and $Br(g)$ are 475 and 655 kJ.mol, what should be the lattice energy of $CsBr(s)$ in $kJ/mol$:

  1. $1120$
  2. $1130$
  3. $1140$
  4. $1150$
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