Which of the following represents an exotherm | vedclass

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Question

(C) An exothermic reaction is one where energy is released,meaning the electron gain enthalpy is negative.$1$. Option $A$ represents the ionization en

Vedclass · Accepted Answer

$O_{(g)} + e^- 	o O_{(g)}^{-}$

Vedclass · Answer

(C) An exothermic reaction is one where energy is released,meaning the electron gain enthalpy is negative.$1$. Option $A$ represents the ionization energy of $F^-$,which is endothermic.$2$. Option $B$ involves adding an electron to $Be$. Since $Be$ has a stable $2s^2$ configuration,adding an electron is endothermic.$3$. Option $C$ represents the first electron gain enthalpy of oxygen,which is exothermic ($O_{(g)} + e^- 	o O_{(g)}^{-}$,$\Delta H = -141 \ kJ/mol$).$4$. Option $D$ represents the formation of $O^{2-}$ from $O$. The addition of the second electron to $O^-$ is endothermic due to inter-electronic repulsion.

List-$I$ (Element)	List-$II$ ($\Delta_{eg}H$ in $kJ \ mol^{-1}$)
$A$. $O$	$I$. $-200$
$B$. $F$	$II$. $-349$
$C$. $Cl$	$III$. $-141$
$D$. $S$	$IV$. $-328$
	$V$. $+48$

Which of the following represents an exothermic reaction?

Similar Questions

Match the following:
List-$I$ (Element) List-$II$ ($\Delta_{eg}H$ in $kJ \ mol^{-1}$)
$A$. $O$ $I$. $-200$
$B$. $F$ $II$. $-349$
$C$. $Cl$ $III$. $-141$
$D$. $S$ $IV$. $-328$
$V$. $+48$

The correct answer is:

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