00. Thermodynamics Terms
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Thermodynamics

272398 For the reaction
$\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{l}), \Delta \mathrm{H}$
$=-285.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$\Delta \mathrm{S}=-0.163 \mathrm{~kJ} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
What is the value of free energy change at $27^{\circ} \mathrm{C}$ for the reaction?

1 $-236.9 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $-281.4 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $-334.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $+334.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Thermodynamics

272399 In a closed insulated container, a liquid is stirred with a paddle to increase its temperature. In this process, which of the following is true?

1 $\Delta \mathrm{E}=\mathrm{W}=\mathrm{Q}=0$
2 $\Delta \mathrm{E} \neq 0, \mathrm{Q}=\mathrm{W}=0$
3 $\Delta \mathrm{E}=\mathrm{W} \neq 0, \mathrm{Q}=0$
4 $\Delta \mathrm{E}=\mathrm{Q} \neq 0, \mathrm{~W}=0$
VITEEE-2019
Thermodynamics

272400 The values of $\Delta H$ and $\Delta S$ for the reaction, $\mathrm{C}$ (graphite) $+\mathrm{CO}_2(\mathrm{~g}) \rightarrow 2 \mathrm{CO}(\mathrm{g})$ are $170 \mathrm{~kJ}$ and $170 \mathrm{JK}^1$, respectively. This reaction will be spontaneous at

1 $910 \mathrm{~K}$
2 $1000 \mathrm{~K}$
3 $510 \mathrm{~K}$
4 $710 \mathrm{~K}$
AIPMT-2009
Thermodynamics

272401 Calculate enthalpy change for the change $8 \mathrm{~S}(\mathrm{~g}) \rightarrow \mathrm{S}_8(\mathrm{~g})$, given that
$\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+2 \mathrm{~S}(\mathrm{~g}), \Delta \mathrm{H}=239.0 \mathrm{k} \mathrm{cal} \mathrm{mol}^{-1}$
$\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+\mathrm{S}(\mathrm{g}), \Delta \mathrm{H}=175.0 \mathrm{k} \mathrm{cal} \mathrm{mol}^{-1}$

1 $+512.0 \mathrm{k} \mathrm{cal}$
2 $-512.0 \mathrm{k} \mathrm{cal}$
3 $508.8 \mathrm{k} \mathrm{cal}$
4 $-508.0 \mathrm{k} \mathrm{cal}$
VITEEE-2018
Thermodynamics

272403 Consider the reaction: $\mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3$ carried out at constant temperature and pressure. If $\Delta H$ and $\Delta U$ are the enthalpy and internal energy changes for the reaction, which of the following expressions is true?

1 $\Delta \mathrm{H}>\Delta \mathrm{U}$
2 $\Delta \mathrm{H}<\Delta \mathrm{U}$
3 $\Delta \mathrm{H}=\Delta \mathrm{U}$
4 $\Delta \mathrm{H}=0$
AIEEE-2005
NEET DIGITAL LIBRARY
Thermodynamics

272398 For the reaction
$\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{l}), \Delta \mathrm{H}$
$=-285.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$\Delta \mathrm{S}=-0.163 \mathrm{~kJ} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
What is the value of free energy change at $27^{\circ} \mathrm{C}$ for the reaction?

1 $-236.9 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $-281.4 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $-334.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $+334.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Thermodynamics

272399 In a closed insulated container, a liquid is stirred with a paddle to increase its temperature. In this process, which of the following is true?

1 $\Delta \mathrm{E}=\mathrm{W}=\mathrm{Q}=0$
2 $\Delta \mathrm{E} \neq 0, \mathrm{Q}=\mathrm{W}=0$
3 $\Delta \mathrm{E}=\mathrm{W} \neq 0, \mathrm{Q}=0$
4 $\Delta \mathrm{E}=\mathrm{Q} \neq 0, \mathrm{~W}=0$
VITEEE-2019
Thermodynamics

272400 The values of $\Delta H$ and $\Delta S$ for the reaction, $\mathrm{C}$ (graphite) $+\mathrm{CO}_2(\mathrm{~g}) \rightarrow 2 \mathrm{CO}(\mathrm{g})$ are $170 \mathrm{~kJ}$ and $170 \mathrm{JK}^1$, respectively. This reaction will be spontaneous at

1 $910 \mathrm{~K}$
2 $1000 \mathrm{~K}$
3 $510 \mathrm{~K}$
4 $710 \mathrm{~K}$
AIPMT-2009
Thermodynamics

272401 Calculate enthalpy change for the change $8 \mathrm{~S}(\mathrm{~g}) \rightarrow \mathrm{S}_8(\mathrm{~g})$, given that
$\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+2 \mathrm{~S}(\mathrm{~g}), \Delta \mathrm{H}=239.0 \mathrm{k} \mathrm{cal} \mathrm{mol}^{-1}$
$\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+\mathrm{S}(\mathrm{g}), \Delta \mathrm{H}=175.0 \mathrm{k} \mathrm{cal} \mathrm{mol}^{-1}$

1 $+512.0 \mathrm{k} \mathrm{cal}$
2 $-512.0 \mathrm{k} \mathrm{cal}$
3 $508.8 \mathrm{k} \mathrm{cal}$
4 $-508.0 \mathrm{k} \mathrm{cal}$
VITEEE-2018
Thermodynamics

272403 Consider the reaction: $\mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3$ carried out at constant temperature and pressure. If $\Delta H$ and $\Delta U$ are the enthalpy and internal energy changes for the reaction, which of the following expressions is true?

1 $\Delta \mathrm{H}>\Delta \mathrm{U}$
2 $\Delta \mathrm{H}<\Delta \mathrm{U}$
3 $\Delta \mathrm{H}=\Delta \mathrm{U}$
4 $\Delta \mathrm{H}=0$
AIEEE-2005
Join With Us for More Updates
Thermodynamics

272398 For the reaction
$\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{l}), \Delta \mathrm{H}$
$=-285.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$\Delta \mathrm{S}=-0.163 \mathrm{~kJ} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
What is the value of free energy change at $27^{\circ} \mathrm{C}$ for the reaction?

1 $-236.9 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $-281.4 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $-334.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $+334.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Thermodynamics

272399 In a closed insulated container, a liquid is stirred with a paddle to increase its temperature. In this process, which of the following is true?

1 $\Delta \mathrm{E}=\mathrm{W}=\mathrm{Q}=0$
2 $\Delta \mathrm{E} \neq 0, \mathrm{Q}=\mathrm{W}=0$
3 $\Delta \mathrm{E}=\mathrm{W} \neq 0, \mathrm{Q}=0$
4 $\Delta \mathrm{E}=\mathrm{Q} \neq 0, \mathrm{~W}=0$
VITEEE-2019
Thermodynamics

272400 The values of $\Delta H$ and $\Delta S$ for the reaction, $\mathrm{C}$ (graphite) $+\mathrm{CO}_2(\mathrm{~g}) \rightarrow 2 \mathrm{CO}(\mathrm{g})$ are $170 \mathrm{~kJ}$ and $170 \mathrm{JK}^1$, respectively. This reaction will be spontaneous at

1 $910 \mathrm{~K}$
2 $1000 \mathrm{~K}$
3 $510 \mathrm{~K}$
4 $710 \mathrm{~K}$
AIPMT-2009
Thermodynamics

272401 Calculate enthalpy change for the change $8 \mathrm{~S}(\mathrm{~g}) \rightarrow \mathrm{S}_8(\mathrm{~g})$, given that
$\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+2 \mathrm{~S}(\mathrm{~g}), \Delta \mathrm{H}=239.0 \mathrm{k} \mathrm{cal} \mathrm{mol}^{-1}$
$\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+\mathrm{S}(\mathrm{g}), \Delta \mathrm{H}=175.0 \mathrm{k} \mathrm{cal} \mathrm{mol}^{-1}$

1 $+512.0 \mathrm{k} \mathrm{cal}$
2 $-512.0 \mathrm{k} \mathrm{cal}$
3 $508.8 \mathrm{k} \mathrm{cal}$
4 $-508.0 \mathrm{k} \mathrm{cal}$
VITEEE-2018
Thermodynamics

272403 Consider the reaction: $\mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3$ carried out at constant temperature and pressure. If $\Delta H$ and $\Delta U$ are the enthalpy and internal energy changes for the reaction, which of the following expressions is true?

1 $\Delta \mathrm{H}>\Delta \mathrm{U}$
2 $\Delta \mathrm{H}<\Delta \mathrm{U}$
3 $\Delta \mathrm{H}=\Delta \mathrm{U}$
4 $\Delta \mathrm{H}=0$
AIEEE-2005
For More Updates join with Us
Thermodynamics

272398 For the reaction
$\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{l}), \Delta \mathrm{H}$
$=-285.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$\Delta \mathrm{S}=-0.163 \mathrm{~kJ} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
What is the value of free energy change at $27^{\circ} \mathrm{C}$ for the reaction?

1 $-236.9 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $-281.4 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $-334.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $+334.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Thermodynamics

272399 In a closed insulated container, a liquid is stirred with a paddle to increase its temperature. In this process, which of the following is true?

1 $\Delta \mathrm{E}=\mathrm{W}=\mathrm{Q}=0$
2 $\Delta \mathrm{E} \neq 0, \mathrm{Q}=\mathrm{W}=0$
3 $\Delta \mathrm{E}=\mathrm{W} \neq 0, \mathrm{Q}=0$
4 $\Delta \mathrm{E}=\mathrm{Q} \neq 0, \mathrm{~W}=0$
VITEEE-2019
Thermodynamics

272400 The values of $\Delta H$ and $\Delta S$ for the reaction, $\mathrm{C}$ (graphite) $+\mathrm{CO}_2(\mathrm{~g}) \rightarrow 2 \mathrm{CO}(\mathrm{g})$ are $170 \mathrm{~kJ}$ and $170 \mathrm{JK}^1$, respectively. This reaction will be spontaneous at

1 $910 \mathrm{~K}$
2 $1000 \mathrm{~K}$
3 $510 \mathrm{~K}$
4 $710 \mathrm{~K}$
AIPMT-2009
Thermodynamics

272401 Calculate enthalpy change for the change $8 \mathrm{~S}(\mathrm{~g}) \rightarrow \mathrm{S}_8(\mathrm{~g})$, given that
$\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+2 \mathrm{~S}(\mathrm{~g}), \Delta \mathrm{H}=239.0 \mathrm{k} \mathrm{cal} \mathrm{mol}^{-1}$
$\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+\mathrm{S}(\mathrm{g}), \Delta \mathrm{H}=175.0 \mathrm{k} \mathrm{cal} \mathrm{mol}^{-1}$

1 $+512.0 \mathrm{k} \mathrm{cal}$
2 $-512.0 \mathrm{k} \mathrm{cal}$
3 $508.8 \mathrm{k} \mathrm{cal}$
4 $-508.0 \mathrm{k} \mathrm{cal}$
VITEEE-2018
Thermodynamics

272403 Consider the reaction: $\mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3$ carried out at constant temperature and pressure. If $\Delta H$ and $\Delta U$ are the enthalpy and internal energy changes for the reaction, which of the following expressions is true?

1 $\Delta \mathrm{H}>\Delta \mathrm{U}$
2 $\Delta \mathrm{H}<\Delta \mathrm{U}$
3 $\Delta \mathrm{H}=\Delta \mathrm{U}$
4 $\Delta \mathrm{H}=0$
AIEEE-2005
NEET DIGITAL LIBRARY
Thermodynamics

272398 For the reaction
$\mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{l}), \Delta \mathrm{H}$
$=-285.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$\Delta \mathrm{S}=-0.163 \mathrm{~kJ} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
What is the value of free energy change at $27^{\circ} \mathrm{C}$ for the reaction?

1 $-236.9 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $-281.4 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $-334.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $+334.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Thermodynamics

272399 In a closed insulated container, a liquid is stirred with a paddle to increase its temperature. In this process, which of the following is true?

1 $\Delta \mathrm{E}=\mathrm{W}=\mathrm{Q}=0$
2 $\Delta \mathrm{E} \neq 0, \mathrm{Q}=\mathrm{W}=0$
3 $\Delta \mathrm{E}=\mathrm{W} \neq 0, \mathrm{Q}=0$
4 $\Delta \mathrm{E}=\mathrm{Q} \neq 0, \mathrm{~W}=0$
VITEEE-2019
Thermodynamics

272400 The values of $\Delta H$ and $\Delta S$ for the reaction, $\mathrm{C}$ (graphite) $+\mathrm{CO}_2(\mathrm{~g}) \rightarrow 2 \mathrm{CO}(\mathrm{g})$ are $170 \mathrm{~kJ}$ and $170 \mathrm{JK}^1$, respectively. This reaction will be spontaneous at

1 $910 \mathrm{~K}$
2 $1000 \mathrm{~K}$
3 $510 \mathrm{~K}$
4 $710 \mathrm{~K}$
AIPMT-2009
Thermodynamics

272401 Calculate enthalpy change for the change $8 \mathrm{~S}(\mathrm{~g}) \rightarrow \mathrm{S}_8(\mathrm{~g})$, given that
$\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+2 \mathrm{~S}(\mathrm{~g}), \Delta \mathrm{H}=239.0 \mathrm{k} \mathrm{cal} \mathrm{mol}^{-1}$
$\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+\mathrm{S}(\mathrm{g}), \Delta \mathrm{H}=175.0 \mathrm{k} \mathrm{cal} \mathrm{mol}^{-1}$

1 $+512.0 \mathrm{k} \mathrm{cal}$
2 $-512.0 \mathrm{k} \mathrm{cal}$
3 $508.8 \mathrm{k} \mathrm{cal}$
4 $-508.0 \mathrm{k} \mathrm{cal}$
VITEEE-2018
Thermodynamics

272403 Consider the reaction: $\mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3$ carried out at constant temperature and pressure. If $\Delta H$ and $\Delta U$ are the enthalpy and internal energy changes for the reaction, which of the following expressions is true?

1 $\Delta \mathrm{H}>\Delta \mathrm{U}$
2 $\Delta \mathrm{H}<\Delta \mathrm{U}$
3 $\Delta \mathrm{H}=\Delta \mathrm{U}$
4 $\Delta \mathrm{H}=0$
AIEEE-2005