00. Thermodynamics Terms
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Thermodynamics

272463 Match List I with List II and select the correct answer using the codes.{l|l}
| List I | List II |
| :--- | :--- |
| A. Spontaneous process | 1 . $\Delta \mathrm{H}<0$ |
| B. Exothermic process | 2. Heat of reaction |
| C. Enthalpy at constant Pressure | 3 . $\Delta \mathrm{G}<0$ |
| D. Cyclic process | 4 . $\Delta \mathrm{U}=0, \Delta \mathrm{H}=0$ |

1 $A \rightarrow 4$
$B \rightarrow 2$
$C \rightarrow 1$
$D \rightarrow 3$
2 $A \rightarrow 3$
$B \rightarrow 1$
$C \rightarrow 2$
$D \rightarrow 4$
3 $A \rightarrow 1$
$B \rightarrow 3$
$C \rightarrow 4$
$D \rightarrow 2$
4 $A \rightarrow 1$
$B \rightarrow 2$
$C \rightarrow 3$
$D \rightarrow 4$
CG PET- 2016
Thermodynamics

272470 In conversion of limestone to lime, $\mathrm{CaCO}_3(\mathrm{~s}) \longrightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_2$ (g) the values of $\Delta H^{\circ}$ and $\Delta \mathrm{S}^{\circ}$ are $+179.1 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $160.2 \mathrm{~J} / \mathrm{K}$, respectively at $298 \mathrm{~K}$ and 1 bar. Assuming that $\Delta H^{\circ}$ and $\Delta S^{\circ}$ do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

1 $1008 \mathrm{~K}$
2 $1200 \mathrm{~K}$
3 $845 \mathrm{~K}$
4 $1118 \mathrm{~K}$
AIEEE-2007
Thermodynamics

272471 The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of $10 \mathrm{dm}^3$ to a volume of 100 $\mathrm{dm}^3$ at $27^{\circ} \mathrm{C}$ is

1 $38.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
2 $35.8 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
3 $32.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
4 $42.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
AIEEE-2011
Thermodynamics

272472 Two blocks of the same metal having same mass and at temperature $T_1$ and $T_2$ respectively, are brought in contact with each other and allowed to attain thermal equilibrium at constant pressure. The change in entropy, $\Delta S$ for this process is

1 $2 \mathrm{C}_{\mathrm{p}} \mathrm{k} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)^{\frac{1}{2}}}{\mathrm{~T}_1 \mathrm{~T}_2}\right]$
2 $2 \mathrm{C}_{\mathrm{p}} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)}{4 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
3 $\mathrm{C}_{\mathrm{p}} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)^2}{4 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
4 $2 \mathrm{C}_{\mathrm{p}} \ln \left[\frac{\mathrm{T}_1+\mathrm{T}_2}{2 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
JEE Main-2019 Shift-I
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Thermodynamics

272463 Match List I with List II and select the correct answer using the codes.{l|l}
| List I | List II |
| :--- | :--- |
| A. Spontaneous process | 1 . $\Delta \mathrm{H}<0$ |
| B. Exothermic process | 2. Heat of reaction |
| C. Enthalpy at constant Pressure | 3 . $\Delta \mathrm{G}<0$ |
| D. Cyclic process | 4 . $\Delta \mathrm{U}=0, \Delta \mathrm{H}=0$ |

1 $A \rightarrow 4$
$B \rightarrow 2$
$C \rightarrow 1$
$D \rightarrow 3$
2 $A \rightarrow 3$
$B \rightarrow 1$
$C \rightarrow 2$
$D \rightarrow 4$
3 $A \rightarrow 1$
$B \rightarrow 3$
$C \rightarrow 4$
$D \rightarrow 2$
4 $A \rightarrow 1$
$B \rightarrow 2$
$C \rightarrow 3$
$D \rightarrow 4$
CG PET- 2016
Thermodynamics

272470 In conversion of limestone to lime, $\mathrm{CaCO}_3(\mathrm{~s}) \longrightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_2$ (g) the values of $\Delta H^{\circ}$ and $\Delta \mathrm{S}^{\circ}$ are $+179.1 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $160.2 \mathrm{~J} / \mathrm{K}$, respectively at $298 \mathrm{~K}$ and 1 bar. Assuming that $\Delta H^{\circ}$ and $\Delta S^{\circ}$ do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

1 $1008 \mathrm{~K}$
2 $1200 \mathrm{~K}$
3 $845 \mathrm{~K}$
4 $1118 \mathrm{~K}$
AIEEE-2007
Thermodynamics

272471 The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of $10 \mathrm{dm}^3$ to a volume of 100 $\mathrm{dm}^3$ at $27^{\circ} \mathrm{C}$ is

1 $38.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
2 $35.8 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
3 $32.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
4 $42.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
AIEEE-2011
Thermodynamics

272472 Two blocks of the same metal having same mass and at temperature $T_1$ and $T_2$ respectively, are brought in contact with each other and allowed to attain thermal equilibrium at constant pressure. The change in entropy, $\Delta S$ for this process is

1 $2 \mathrm{C}_{\mathrm{p}} \mathrm{k} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)^{\frac{1}{2}}}{\mathrm{~T}_1 \mathrm{~T}_2}\right]$
2 $2 \mathrm{C}_{\mathrm{p}} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)}{4 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
3 $\mathrm{C}_{\mathrm{p}} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)^2}{4 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
4 $2 \mathrm{C}_{\mathrm{p}} \ln \left[\frac{\mathrm{T}_1+\mathrm{T}_2}{2 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
JEE Main-2019 Shift-I
NEET DIGITAL LIBRARY
Thermodynamics

272463 Match List I with List II and select the correct answer using the codes.{l|l}
| List I | List II |
| :--- | :--- |
| A. Spontaneous process | 1 . $\Delta \mathrm{H}<0$ |
| B. Exothermic process | 2. Heat of reaction |
| C. Enthalpy at constant Pressure | 3 . $\Delta \mathrm{G}<0$ |
| D. Cyclic process | 4 . $\Delta \mathrm{U}=0, \Delta \mathrm{H}=0$ |

1 $A \rightarrow 4$
$B \rightarrow 2$
$C \rightarrow 1$
$D \rightarrow 3$
2 $A \rightarrow 3$
$B \rightarrow 1$
$C \rightarrow 2$
$D \rightarrow 4$
3 $A \rightarrow 1$
$B \rightarrow 3$
$C \rightarrow 4$
$D \rightarrow 2$
4 $A \rightarrow 1$
$B \rightarrow 2$
$C \rightarrow 3$
$D \rightarrow 4$
CG PET- 2016
Thermodynamics

272470 In conversion of limestone to lime, $\mathrm{CaCO}_3(\mathrm{~s}) \longrightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_2$ (g) the values of $\Delta H^{\circ}$ and $\Delta \mathrm{S}^{\circ}$ are $+179.1 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $160.2 \mathrm{~J} / \mathrm{K}$, respectively at $298 \mathrm{~K}$ and 1 bar. Assuming that $\Delta H^{\circ}$ and $\Delta S^{\circ}$ do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

1 $1008 \mathrm{~K}$
2 $1200 \mathrm{~K}$
3 $845 \mathrm{~K}$
4 $1118 \mathrm{~K}$
AIEEE-2007
Thermodynamics

272471 The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of $10 \mathrm{dm}^3$ to a volume of 100 $\mathrm{dm}^3$ at $27^{\circ} \mathrm{C}$ is

1 $38.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
2 $35.8 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
3 $32.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
4 $42.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
AIEEE-2011
Thermodynamics

272472 Two blocks of the same metal having same mass and at temperature $T_1$ and $T_2$ respectively, are brought in contact with each other and allowed to attain thermal equilibrium at constant pressure. The change in entropy, $\Delta S$ for this process is

1 $2 \mathrm{C}_{\mathrm{p}} \mathrm{k} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)^{\frac{1}{2}}}{\mathrm{~T}_1 \mathrm{~T}_2}\right]$
2 $2 \mathrm{C}_{\mathrm{p}} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)}{4 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
3 $\mathrm{C}_{\mathrm{p}} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)^2}{4 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
4 $2 \mathrm{C}_{\mathrm{p}} \ln \left[\frac{\mathrm{T}_1+\mathrm{T}_2}{2 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
JEE Main-2019 Shift-I
Join With Us for More Updates
Thermodynamics

272463 Match List I with List II and select the correct answer using the codes.{l|l}
| List I | List II |
| :--- | :--- |
| A. Spontaneous process | 1 . $\Delta \mathrm{H}<0$ |
| B. Exothermic process | 2. Heat of reaction |
| C. Enthalpy at constant Pressure | 3 . $\Delta \mathrm{G}<0$ |
| D. Cyclic process | 4 . $\Delta \mathrm{U}=0, \Delta \mathrm{H}=0$ |

1 $A \rightarrow 4$
$B \rightarrow 2$
$C \rightarrow 1$
$D \rightarrow 3$
2 $A \rightarrow 3$
$B \rightarrow 1$
$C \rightarrow 2$
$D \rightarrow 4$
3 $A \rightarrow 1$
$B \rightarrow 3$
$C \rightarrow 4$
$D \rightarrow 2$
4 $A \rightarrow 1$
$B \rightarrow 2$
$C \rightarrow 3$
$D \rightarrow 4$
CG PET- 2016
Thermodynamics

272470 In conversion of limestone to lime, $\mathrm{CaCO}_3(\mathrm{~s}) \longrightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_2$ (g) the values of $\Delta H^{\circ}$ and $\Delta \mathrm{S}^{\circ}$ are $+179.1 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $160.2 \mathrm{~J} / \mathrm{K}$, respectively at $298 \mathrm{~K}$ and 1 bar. Assuming that $\Delta H^{\circ}$ and $\Delta S^{\circ}$ do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

1 $1008 \mathrm{~K}$
2 $1200 \mathrm{~K}$
3 $845 \mathrm{~K}$
4 $1118 \mathrm{~K}$
AIEEE-2007
Thermodynamics

272471 The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of $10 \mathrm{dm}^3$ to a volume of 100 $\mathrm{dm}^3$ at $27^{\circ} \mathrm{C}$ is

1 $38.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
2 $35.8 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
3 $32.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
4 $42.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
AIEEE-2011
Thermodynamics

272472 Two blocks of the same metal having same mass and at temperature $T_1$ and $T_2$ respectively, are brought in contact with each other and allowed to attain thermal equilibrium at constant pressure. The change in entropy, $\Delta S$ for this process is

1 $2 \mathrm{C}_{\mathrm{p}} \mathrm{k} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)^{\frac{1}{2}}}{\mathrm{~T}_1 \mathrm{~T}_2}\right]$
2 $2 \mathrm{C}_{\mathrm{p}} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)}{4 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
3 $\mathrm{C}_{\mathrm{p}} \ln \left[\frac{\left(\mathrm{T}_1+\mathrm{T}_2\right)^2}{4 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
4 $2 \mathrm{C}_{\mathrm{p}} \ln \left[\frac{\mathrm{T}_1+\mathrm{T}_2}{2 \mathrm{~T}_1 \mathrm{~T}_2}\right]$
JEE Main-2019 Shift-I
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