272324 Which of the following options are correct?
| Options | $ ^{}$ | $ ^{}$ | $ ^{}$ | Spontaneity of the reaction |
|---|---|---|---|---|
|A | + | + | + | Spontaneous at low T |
|B | + | + | - | Spontaneous at high $$ |
|C | - | - | - | Spontaneous at low T |
|D | + | - | + | Spontaneous at high T |
|

272325 Consider the following :
$\mathrm{Mg}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_2(\mathrm{aq})+\mathrm{H}_2(\mathrm{~g})$
$\Delta \mathrm{H}=-467 \mathrm{kJmol}$
$\mathrm{MgO}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_2(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l)$
$\Delta \mathrm{H}=-151 \mathrm{kJmol}^{-1}$
$\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(I)$
and given that for water,
$\Delta \mathrm{H}_{\mathrm{f}}^0=-286 \mathrm{kJmol}^{-1}$
What is $\Delta \mathrm{H}_{\mathrm{f}}^{\circ}$ for $\mathrm{MgO}$ (s)?

272326 An ideal gas at initial pressure $p_i$ and volume $V_i$ undergoes reversible expansion to the same volume $V_{\mathrm{f}}$ either isothermally or adiabatically. Consider the following statements:
1.$\mathrm{P}_{\mathrm{f}}$ (adiabatic) $<\mathrm{P}_{\mathrm{f}}$ (isothermal)
2.$\mid W$ (adiabatic) $|<| W$ (isothermal) $\mid$
3.$\mathrm{T}_{\mathrm{f}}$ (adiabatic) $<\mathrm{T}_{\mathrm{f}}$ (isothermal)
4.$\mid q$ (adiabatic) $|<| q$ (isothermal) $\mid$

272330 In the reaction,
$4 \mathrm{NO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{~N}_2 \mathrm{O}_5(\mathrm{~g}), \Delta \mathrm{H}=-111 \mathrm{~kJ}$
If $\mathrm{N}_2 \mathrm{O}_5(\mathrm{~s})$ is formed instead of $\mathrm{N}_2 \mathrm{O}_5(\mathrm{~g})$, the $\Delta \mathrm{H}$ value in $\mathrm{kJ}$ is
$\left(\Delta \mathrm{H}_{\text {sablimation }}\right.$ for $\left.\mathrm{N}_2 \mathrm{O}_5=54 \mathrm{~kJ} \mathrm{~mol} \mathrm{~m}^{-1}\right)$

272324 Which of the following options are correct?
| Options | $ ^{}$ | $ ^{}$ | $ ^{}$ | Spontaneity of the reaction |
|---|---|---|---|---|
|A | + | + | + | Spontaneous at low T |
|B | + | + | - | Spontaneous at high $$ |
|C | - | - | - | Spontaneous at low T |
|D | + | - | + | Spontaneous at high T |
|

272325 Consider the following :
$\mathrm{Mg}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_2(\mathrm{aq})+\mathrm{H}_2(\mathrm{~g})$
$\Delta \mathrm{H}=-467 \mathrm{kJmol}$
$\mathrm{MgO}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_2(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l)$
$\Delta \mathrm{H}=-151 \mathrm{kJmol}^{-1}$
$\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(I)$
and given that for water,
$\Delta \mathrm{H}_{\mathrm{f}}^0=-286 \mathrm{kJmol}^{-1}$
What is $\Delta \mathrm{H}_{\mathrm{f}}^{\circ}$ for $\mathrm{MgO}$ (s)?

272326 An ideal gas at initial pressure $p_i$ and volume $V_i$ undergoes reversible expansion to the same volume $V_{\mathrm{f}}$ either isothermally or adiabatically. Consider the following statements:
1.$\mathrm{P}_{\mathrm{f}}$ (adiabatic) $<\mathrm{P}_{\mathrm{f}}$ (isothermal)
2.$\mid W$ (adiabatic) $|<| W$ (isothermal) $\mid$
3.$\mathrm{T}_{\mathrm{f}}$ (adiabatic) $<\mathrm{T}_{\mathrm{f}}$ (isothermal)
4.$\mid q$ (adiabatic) $|<| q$ (isothermal) $\mid$

272330 In the reaction,
$4 \mathrm{NO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{~N}_2 \mathrm{O}_5(\mathrm{~g}), \Delta \mathrm{H}=-111 \mathrm{~kJ}$
If $\mathrm{N}_2 \mathrm{O}_5(\mathrm{~s})$ is formed instead of $\mathrm{N}_2 \mathrm{O}_5(\mathrm{~g})$, the $\Delta \mathrm{H}$ value in $\mathrm{kJ}$ is
$\left(\Delta \mathrm{H}_{\text {sablimation }}\right.$ for $\left.\mathrm{N}_2 \mathrm{O}_5=54 \mathrm{~kJ} \mathrm{~mol} \mathrm{~m}^{-1}\right)$

272324 Which of the following options are correct?
| Options | $ ^{}$ | $ ^{}$ | $ ^{}$ | Spontaneity of the reaction |
|---|---|---|---|---|
|A | + | + | + | Spontaneous at low T |
|B | + | + | - | Spontaneous at high $$ |
|C | - | - | - | Spontaneous at low T |
|D | + | - | + | Spontaneous at high T |
|

272325 Consider the following :
$\mathrm{Mg}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_2(\mathrm{aq})+\mathrm{H}_2(\mathrm{~g})$
$\Delta \mathrm{H}=-467 \mathrm{kJmol}$
$\mathrm{MgO}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_2(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l)$
$\Delta \mathrm{H}=-151 \mathrm{kJmol}^{-1}$
$\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(I)$
and given that for water,
$\Delta \mathrm{H}_{\mathrm{f}}^0=-286 \mathrm{kJmol}^{-1}$
What is $\Delta \mathrm{H}_{\mathrm{f}}^{\circ}$ for $\mathrm{MgO}$ (s)?

272326 An ideal gas at initial pressure $p_i$ and volume $V_i$ undergoes reversible expansion to the same volume $V_{\mathrm{f}}$ either isothermally or adiabatically. Consider the following statements:
1.$\mathrm{P}_{\mathrm{f}}$ (adiabatic) $<\mathrm{P}_{\mathrm{f}}$ (isothermal)
2.$\mid W$ (adiabatic) $|<| W$ (isothermal) $\mid$
3.$\mathrm{T}_{\mathrm{f}}$ (adiabatic) $<\mathrm{T}_{\mathrm{f}}$ (isothermal)
4.$\mid q$ (adiabatic) $|<| q$ (isothermal) $\mid$

272330 In the reaction,
$4 \mathrm{NO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{~N}_2 \mathrm{O}_5(\mathrm{~g}), \Delta \mathrm{H}=-111 \mathrm{~kJ}$
If $\mathrm{N}_2 \mathrm{O}_5(\mathrm{~s})$ is formed instead of $\mathrm{N}_2 \mathrm{O}_5(\mathrm{~g})$, the $\Delta \mathrm{H}$ value in $\mathrm{kJ}$ is
$\left(\Delta \mathrm{H}_{\text {sablimation }}\right.$ for $\left.\mathrm{N}_2 \mathrm{O}_5=54 \mathrm{~kJ} \mathrm{~mol} \mathrm{~m}^{-1}\right)$

272324 Which of the following options are correct?
| Options | $ ^{}$ | $ ^{}$ | $ ^{}$ | Spontaneity of the reaction |
|---|---|---|---|---|
|A | + | + | + | Spontaneous at low T |
|B | + | + | - | Spontaneous at high $$ |
|C | - | - | - | Spontaneous at low T |
|D | + | - | + | Spontaneous at high T |
|

272325 Consider the following :
$\mathrm{Mg}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_2(\mathrm{aq})+\mathrm{H}_2(\mathrm{~g})$
$\Delta \mathrm{H}=-467 \mathrm{kJmol}$
$\mathrm{MgO}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_2(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l)$
$\Delta \mathrm{H}=-151 \mathrm{kJmol}^{-1}$
$\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(I)$
and given that for water,
$\Delta \mathrm{H}_{\mathrm{f}}^0=-286 \mathrm{kJmol}^{-1}$
What is $\Delta \mathrm{H}_{\mathrm{f}}^{\circ}$ for $\mathrm{MgO}$ (s)?

272326 An ideal gas at initial pressure $p_i$ and volume $V_i$ undergoes reversible expansion to the same volume $V_{\mathrm{f}}$ either isothermally or adiabatically. Consider the following statements:
1.$\mathrm{P}_{\mathrm{f}}$ (adiabatic) $<\mathrm{P}_{\mathrm{f}}$ (isothermal)
2.$\mid W$ (adiabatic) $|<| W$ (isothermal) $\mid$
3.$\mathrm{T}_{\mathrm{f}}$ (adiabatic) $<\mathrm{T}_{\mathrm{f}}$ (isothermal)
4.$\mid q$ (adiabatic) $|<| q$ (isothermal) $\mid$

272330 In the reaction,
$4 \mathrm{NO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{~N}_2 \mathrm{O}_5(\mathrm{~g}), \Delta \mathrm{H}=-111 \mathrm{~kJ}$
If $\mathrm{N}_2 \mathrm{O}_5(\mathrm{~s})$ is formed instead of $\mathrm{N}_2 \mathrm{O}_5(\mathrm{~g})$, the $\Delta \mathrm{H}$ value in $\mathrm{kJ}$ is
$\left(\Delta \mathrm{H}_{\text {sablimation }}\right.$ for $\left.\mathrm{N}_2 \mathrm{O}_5=54 \mathrm{~kJ} \mathrm{~mol} \mathrm{~m}^{-1}\right)$