(B) We are given the following thermochemical equations:$(1) \ C(\text{graphite}) + O_{2(g)} \to CO_{2(g)}; \Delta H_1 = x \ kJ \ mol^{-1}$$(2) \ C(\t

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(B) We are given the following thermochemical equations:$(1) \ C(\text{graphite}) + O_{2(g)} \to CO_{2(g)}; \Delta H_1 = x \ kJ \ mol^{-1}$$(2) \ C(\text{diamond}) + O_{2(g)} \to CO_{2(g)}; \Delta H_2 = y \ kJ \ mol^{-1}$To find the heat of transition for $C(\text{graphite}) \to C(\text{diamond})$,we subtract equation $(2)$ from equation $(1)$:$C(\text{graphite}) - C(\text{diamond}) = x - y$$C(\text{graphite}) \to C(\text{diamond}); \Delta H_t = (x - y) \ kJ \ mol^{-1}$

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

Medium

The heat of transition $(\Delta H_t)$ of graphite into diamond would be,where
$C(\text{graphite}) + O_{2(g)} \to CO_{2(g)}; \Delta H = x \ kJ \ mol^{-1}$
$C(\text{diamond}) + O_{2(g)} \to CO_{2(g)}; \Delta H = y \ kJ \ mol^{-1}$

A
$(x + y) \ kJ \ mol^{-1}$
B
$(x - y) \ kJ \ mol^{-1}$
C
$(y - x) \ kJ \ mol^{-1}$
D
None of these

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Class 11 Questions

Class 11

Chemistry Questions

Chapter

Thermodynamics

Subtopic

Heat of reaction, Bond energy and Hess law

The enthalpy of combustion of propane,graphite and dihydrogen at $298 \ K$ are: $-2220.0 \ kJ \ mol^{-1}$,$-393.5 \ kJ \ mol^{-1}$ and $-285.8 \ kJ \ mol^{-1}$ respectively. The magnitude of the enthalpy of formation of propane $(C_{3}H_{8})$ is ......... $kJ \ mol^{-1}$. (Nearest integer)

MediumJEE MAIN 2022

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If heat of neutralization is $-13.7 \, KCal$ at $25 \, ^oC$ and $\Delta H_f^o (H_2O) = -68 \, KCal$,then the standard enthalpy of formation of $OH^{-}$ will be.....$KCal$. (in $.3$)

Medium

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If the enthalpy change during the combustion of benzene is $-3264.6 \ kJ/mol$,then the heat produced by the combustion of $39 \ g$ of benzene is ...... $kJ$.

Medium

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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?

Easy

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If the bond dissociation energies of $XY$,$X_2$,and $Y_2$ (all diatomic molecules) are in the ratio of $1 : 1 : 0.5$ and $\Delta_f H$ for the formation of $XY$ is $-200 \ kJ \ mol^{-1}$,the bond dissociation energy of $X_2$ will be in $kJ \ mol^{-1}$:

DifficultAIEEE 2005

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The heat of transition $(\Delta H_t)$ of graphite into diamond would be,where$C(\text{graphite}) + O_{2(g)} \to CO_{2(g)}; \Delta H = x \ kJ \ mol^{-1}$$C(\text{diamond}) + O_{2(g)} \to CO_{2(g)}; \Delta H = y \ kJ \ mol^{-1}$

Similar Questions

The enthalpy of combustion of propane,graphite and dihydrogen at $298 \ K$ are: $-2220.0 \ kJ \ mol^{-1}$,$-393.5 \ kJ \ mol^{-1}$ and $-285.8 \ kJ \ mol^{-1}$ respectively. The magnitude of the enthalpy of formation of propane $(C_{3}H_{8})$ is ......... $kJ \ mol^{-1}$. (Nearest integer)

If heat of neutralization is $-13.7 \, KCal$ at $25 \, ^oC$ and $\Delta H_f^o (H_2O) = -68 \, KCal$,then the standard enthalpy of formation of $OH^{-}$ will be.....$KCal$. (in $.3$)

If the enthalpy change during the combustion of benzene is $-3264.6 \ kJ/mol$,then the heat produced by the combustion of $39 \ g$ of benzene is ...... $kJ$.

$CH_4 + \frac{1}{2}O_2 \to CH_3OH$ 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?

If the bond dissociation energies of $XY$,$X_2$,and $Y_2$ (all diatomic molecules) are in the ratio of $1 : 1 : 0.5$ and $\Delta_f H$ for the formation of $XY$ is $-200 \ kJ \ mol^{-1}$,the bond dissociation energy of $X_2$ will be in $kJ \ mol^{-1}$:

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The heat of transition $(\Delta H_t)$ of graphite into diamond would be,where
$C(\text{graphite}) + O_{2(g)} \to CO_{2(g)}; \Delta H = x \ kJ \ mol^{-1}$
$C(\text{diamond}) + O_{2(g)} \to CO_{2(g)}; \Delta H = y \ kJ \ mol^{-1}$