03. Heat of Reaction
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Thermodynamics

272787 The enthalpy of formation of two compounds $\mathrm{X}$ and $Y$ are $-36 \mathrm{~kJ}$ and $-72 \mathrm{~kJ}$ respectively, which one of the following statement is correct?

1 Compound $\mathrm{X}$ is more stable than compound $\mathrm{Y}$
2 Compound $Y$ is more stable than compound $\mathrm{X}$
3 Both compound $\mathrm{X}$ and $\mathrm{Y}$ are endothermic compounds.
4 Both $\mathrm{X}$ and $\mathrm{y}$ are unstable.
COMEDK-2011
Thermodynamics

272773 Given that,
(i) $\mathrm{CH}_3 \mathrm{CHO}+\frac{5}{2} \mathrm{O}_2 \rightarrow 2 \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$;
$\Delta \mathrm{H}=-1168 \mathrm{~kJ} \mathrm{~mol}-1$
(ii) $\mathrm{CH}_3 \mathrm{COOH}+2 \mathrm{O}_2 \rightarrow 2 \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$
$\Delta \mathrm{H}=-876 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$\Delta \mathrm{H}$ for the reaction,
$\mathrm{CH}_3 \mathrm{CHO}+\frac{1}{2} \mathrm{O}_2 \rightarrow \mathrm{CH}_3 \mathrm{COOH}$, is

1 $-292 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}$
2 $378 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $195 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $-2044 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(A.P.EAMCET-1994)
Thermodynamics

272774 Calculate the heat of formation $(\Delta \mathrm{H})$ of $\mathrm{CO}$ (in kcal) from the following data.
I. $\mathrm{C}_{\text {(graptire) }}+\mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}_2(\mathrm{~g})$;
$\Delta \mathrm{H}=-94 \mathrm{kcal}$
II. $\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}_2(\mathrm{~g})$;

1 -1.3
2 -26
3 -162
4 -82
(A.P.EAMCET-2000)
Thermodynamics

272776 The heat of combustion of $\mathrm{CH}_4, \mathrm{C}$ (graphite) and $\mathrm{H}_2$ (g) are respectively 20 kcal, -40 kcal and -10 kcal. The heat of formation of $\mathrm{CH}_4$ is

1 $-40 \mathrm{kcal}$
2 $+40 \mathrm{kcal}$
3 $80 \mathrm{kcal}$
4 None of these
(A.P.EAMCET-1998)
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Thermodynamics

272787 The enthalpy of formation of two compounds $\mathrm{X}$ and $Y$ are $-36 \mathrm{~kJ}$ and $-72 \mathrm{~kJ}$ respectively, which one of the following statement is correct?

1 Compound $\mathrm{X}$ is more stable than compound $\mathrm{Y}$
2 Compound $Y$ is more stable than compound $\mathrm{X}$
3 Both compound $\mathrm{X}$ and $\mathrm{Y}$ are endothermic compounds.
4 Both $\mathrm{X}$ and $\mathrm{y}$ are unstable.
COMEDK-2011
Thermodynamics

272773 Given that,
(i) $\mathrm{CH}_3 \mathrm{CHO}+\frac{5}{2} \mathrm{O}_2 \rightarrow 2 \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$;
$\Delta \mathrm{H}=-1168 \mathrm{~kJ} \mathrm{~mol}-1$
(ii) $\mathrm{CH}_3 \mathrm{COOH}+2 \mathrm{O}_2 \rightarrow 2 \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$
$\Delta \mathrm{H}=-876 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$\Delta \mathrm{H}$ for the reaction,
$\mathrm{CH}_3 \mathrm{CHO}+\frac{1}{2} \mathrm{O}_2 \rightarrow \mathrm{CH}_3 \mathrm{COOH}$, is

1 $-292 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}$
2 $378 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $195 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $-2044 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(A.P.EAMCET-1994)
Thermodynamics

272774 Calculate the heat of formation $(\Delta \mathrm{H})$ of $\mathrm{CO}$ (in kcal) from the following data.
I. $\mathrm{C}_{\text {(graptire) }}+\mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}_2(\mathrm{~g})$;
$\Delta \mathrm{H}=-94 \mathrm{kcal}$
II. $\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}_2(\mathrm{~g})$;

1 -1.3
2 -26
3 -162
4 -82
(A.P.EAMCET-2000)
Thermodynamics

272776 The heat of combustion of $\mathrm{CH}_4, \mathrm{C}$ (graphite) and $\mathrm{H}_2$ (g) are respectively 20 kcal, -40 kcal and -10 kcal. The heat of formation of $\mathrm{CH}_4$ is

1 $-40 \mathrm{kcal}$
2 $+40 \mathrm{kcal}$
3 $80 \mathrm{kcal}$
4 None of these
(A.P.EAMCET-1998)
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Thermodynamics

272787 The enthalpy of formation of two compounds $\mathrm{X}$ and $Y$ are $-36 \mathrm{~kJ}$ and $-72 \mathrm{~kJ}$ respectively, which one of the following statement is correct?

1 Compound $\mathrm{X}$ is more stable than compound $\mathrm{Y}$
2 Compound $Y$ is more stable than compound $\mathrm{X}$
3 Both compound $\mathrm{X}$ and $\mathrm{Y}$ are endothermic compounds.
4 Both $\mathrm{X}$ and $\mathrm{y}$ are unstable.
COMEDK-2011
Thermodynamics

272773 Given that,
(i) $\mathrm{CH}_3 \mathrm{CHO}+\frac{5}{2} \mathrm{O}_2 \rightarrow 2 \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$;
$\Delta \mathrm{H}=-1168 \mathrm{~kJ} \mathrm{~mol}-1$
(ii) $\mathrm{CH}_3 \mathrm{COOH}+2 \mathrm{O}_2 \rightarrow 2 \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$
$\Delta \mathrm{H}=-876 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$\Delta \mathrm{H}$ for the reaction,
$\mathrm{CH}_3 \mathrm{CHO}+\frac{1}{2} \mathrm{O}_2 \rightarrow \mathrm{CH}_3 \mathrm{COOH}$, is

1 $-292 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}$
2 $378 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $195 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $-2044 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(A.P.EAMCET-1994)
Thermodynamics

272774 Calculate the heat of formation $(\Delta \mathrm{H})$ of $\mathrm{CO}$ (in kcal) from the following data.
I. $\mathrm{C}_{\text {(graptire) }}+\mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}_2(\mathrm{~g})$;
$\Delta \mathrm{H}=-94 \mathrm{kcal}$
II. $\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}_2(\mathrm{~g})$;

1 -1.3
2 -26
3 -162
4 -82
(A.P.EAMCET-2000)
Thermodynamics

272776 The heat of combustion of $\mathrm{CH}_4, \mathrm{C}$ (graphite) and $\mathrm{H}_2$ (g) are respectively 20 kcal, -40 kcal and -10 kcal. The heat of formation of $\mathrm{CH}_4$ is

1 $-40 \mathrm{kcal}$
2 $+40 \mathrm{kcal}$
3 $80 \mathrm{kcal}$
4 None of these
(A.P.EAMCET-1998)
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Thermodynamics

272787 The enthalpy of formation of two compounds $\mathrm{X}$ and $Y$ are $-36 \mathrm{~kJ}$ and $-72 \mathrm{~kJ}$ respectively, which one of the following statement is correct?

1 Compound $\mathrm{X}$ is more stable than compound $\mathrm{Y}$
2 Compound $Y$ is more stable than compound $\mathrm{X}$
3 Both compound $\mathrm{X}$ and $\mathrm{Y}$ are endothermic compounds.
4 Both $\mathrm{X}$ and $\mathrm{y}$ are unstable.
COMEDK-2011
Thermodynamics

272773 Given that,
(i) $\mathrm{CH}_3 \mathrm{CHO}+\frac{5}{2} \mathrm{O}_2 \rightarrow 2 \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$;
$\Delta \mathrm{H}=-1168 \mathrm{~kJ} \mathrm{~mol}-1$
(ii) $\mathrm{CH}_3 \mathrm{COOH}+2 \mathrm{O}_2 \rightarrow 2 \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$
$\Delta \mathrm{H}=-876 \mathrm{~kJ} \mathrm{~mol}^{-1}$
$\Delta \mathrm{H}$ for the reaction,
$\mathrm{CH}_3 \mathrm{CHO}+\frac{1}{2} \mathrm{O}_2 \rightarrow \mathrm{CH}_3 \mathrm{COOH}$, is

1 $-292 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}$
2 $378 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $195 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $-2044 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(A.P.EAMCET-1994)
Thermodynamics

272774 Calculate the heat of formation $(\Delta \mathrm{H})$ of $\mathrm{CO}$ (in kcal) from the following data.
I. $\mathrm{C}_{\text {(graptire) }}+\mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}_2(\mathrm{~g})$;
$\Delta \mathrm{H}=-94 \mathrm{kcal}$
II. $\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{CO}_2(\mathrm{~g})$;

1 -1.3
2 -26
3 -162
4 -82
(A.P.EAMCET-2000)
Thermodynamics

272776 The heat of combustion of $\mathrm{CH}_4, \mathrm{C}$ (graphite) and $\mathrm{H}_2$ (g) are respectively 20 kcal, -40 kcal and -10 kcal. The heat of formation of $\mathrm{CH}_4$ is

1 $-40 \mathrm{kcal}$
2 $+40 \mathrm{kcal}$
3 $80 \mathrm{kcal}$
4 None of these
(A.P.EAMCET-1998)
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