(B) The combustion reactions are:$(1)$ $CH_4(g) + 2O_2(g) \to CO_2(g) + 2H_2O(l)$; $\Delta H = x$$(2)$ $CH_3OH(l) + \frac{3}{2}O_2(g) \to CO_2(g) + 2H

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(B) The combustion reactions are:$(1)$ $CH_4(g) + 2O_2(g) \to CO_2(g) + 2H_2O(l)$; $\Delta H = x$$(2)$ $CH_3OH(l) + \frac{3}{2}O_2(g) \to CO_2(g) + 2H_2O(l)$; $\Delta H = y$Subtracting equation $(2)$ from $(1)$:$(CH_4 + 2O_2) - (CH_3OH + \frac{3}{2}O_2) = x - y$$CH_4 + \frac{1}{2}O_2 \to CH_3OH$; $\Delta H = x - y$Since the reaction is exothermic,$\Delta H < 0$,which implies $x - y < 0$,or $x < y$.

Class 11 Chemistry Thermodynamics Heat of reaction, Bond energy and Hess law

Easy

$CH_4 + \frac{1}{2}O_2 \to CH_3OH$ is an exothermic reaction $(\Delta H < 0)$. If the enthalpies of combustion of $CH_4$ and $CH_3OH$ are $x$ and $y$ respectively,which of the following relations is correct?

A
$x > y$
B
$x < y$
C
$x = y$
D
$x \geq y$

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Class 11

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Chapter

Thermodynamics

Subtopic

Heat of reaction, Bond energy and Hess law

Which of the following reactions defines the standard enthalpy of combustion,$\Delta H_c^ \circ$?

Medium

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The $\Delta H_f^o$ for $CO_{2(g)}$,$CO_{(g)}$ and $H_2O_{(g)}$ are $-393.5$,$-110.5$ and $-241.8 \ kJ \ mol^{-1}$ respectively. The standard enthalpy change (in $kJ$) for the reaction $CO_{2(g)} + H_{2(g)} \to CO_{(g)} + H_2O_{(g)}$ is

MediumAIIMS 2013

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If the ratio of bond dissociation energies of $XY$,$X_2$,and $Y_2$ is $1 : 1 : 0.5$ and the enthalpy of formation of $XY$ is $\Delta_f H = -200 \ kJ \ mol^{-1}$,then the bond dissociation energy of $X_2$ in $kJ \ mol^{-1}$ is:

Medium

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For the reaction $H_{2(g)} + C_{2}H_{4(g)} \rightarrow C_{2}H_{6(g)}$,the enthalpy change is ....... $Kcal \, mol^{-1}$. Given bond energies: $H-H = 103$,$C-H = 99$,$C-C = 80$,and $C=C = 145 \, Kcal \, mol^{-1}$.

Medium

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The heat of neutralisation of a strong acid and a strong alkali is $57.0 \, kJ \, mol^{-1}$. The heat released when $0.5 \, mole$ of $HNO_3$ solution is mixed with $0.2 \, mole$ of $KOH$ is $...... \, kJ$.

MediumAIIMS 2002

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$CH_4 + \frac{1}{2}O_2 \to CH_3OH$ is an exothermic reaction $(\Delta H < 0)$. If the enthalpies of combustion of $CH_4$ and $CH_3OH$ are $x$ and $y$ respectively,which of the following relations is correct?

Similar Questions

Which of the following reactions defines the standard enthalpy of combustion,$\Delta H_c^ \circ$?

The $\Delta H_f^o$ for $CO_{2(g)}$,$CO_{(g)}$ and $H_2O_{(g)}$ are $-393.5$,$-110.5$ and $-241.8 \ kJ \ mol^{-1}$ respectively. The standard enthalpy change (in $kJ$) for the reaction $CO_{2(g)} + H_{2(g)} \to CO_{(g)} + H_2O_{(g)}$ is

If the ratio of bond dissociation energies of $XY$,$X_2$,and $Y_2$ is $1 : 1 : 0.5$ and the enthalpy of formation of $XY$ is $\Delta_f H = -200 \ kJ \ mol^{-1}$,then the bond dissociation energy of $X_2$ in $kJ \ mol^{-1}$ is:

For the reaction $H_{2(g)} + C_{2}H_{4(g)} \rightarrow C_{2}H_{6(g)}$,the enthalpy change is ....... $Kcal \, mol^{-1}$. Given bond energies: $H-H = 103$,$C-H = 99$,$C-C = 80$,and $C=C = 145 \, Kcal \, mol^{-1}$.

The heat of neutralisation of a strong acid and a strong alkali is $57.0 \, kJ \, mol^{-1}$. The heat released when $0.5 \, mole$ of $HNO_3$ solution is mixed with $0.2 \, mole$ of $KOH$ is $...... \, kJ$.

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