Select the process in which the least enthalp | vedclass

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(B) The enthalpy changes for the given processes are as follows:$1$. $O_{(g)} 	o O^{+}_{(g)}$: This is the first ionization enthalpy of oxygen,which

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$O_{(g)} 	o O^{-}_{(g)}$

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(B) The enthalpy changes for the given processes are as follows:$1$. $O_{(g)} 	o O^{+}_{(g)}$: This is the first ionization enthalpy of oxygen,which is a large positive value $(+1314 \ kJ/mol)$.$2$. $O_{(g)} 	o O^{-}_{(g)}$: This is the electron gain enthalpy of oxygen,which is negative $(-141 \ kJ/mol)$.$3$. $O^{+}_{(g)} 	o O^{2+}_{(g)}$: This is the second ionization enthalpy of oxygen,which is a very large positive value $(+3388 \ kJ/mol)$.$4$. $S_{(g)} 	o S^{-}_{(g)}$: This is the electron gain enthalpy of sulfur,which is negative $(-200 \ kJ/mol)$.Comparing the magnitudes of enthalpy change,the process $O_{(g)} 	o O^{-}_{(g)}$ involves the release of $141 \ kJ/mol$,while $S_{(g)} 	o S^{-}_{(g)}$ involves the release of $200 \ kJ/mol$. The process with the least enthalpy change (smallest absolute value) is $O_{(g)} 	o O^{-}_{(g)}$.

Select the process in which the least enthalpy change is associated:

Similar Questions

When an electron is added to elements of group $16$ and $17$ in $n = 2$ and $n = 3$ shells,which case experiences less electron-electron repulsion and why?

Electronic configurations of four elements $A, B, C$ and $D$ are given below :
$(A)$ $1s^2 2s^2 2p^6$
$(B)$ $1s^2 2s^2 2p^4$
$(C)$ $1s^2 2s^2 2p^6 3s^1$
$(D)$ $1s^2 2s^2 2p^5$
Which of the following is the correct order of increasing tendency to gain electron :

The correct order of electron gain enthalpy of $N$,$O$,$Cl$,$Al$ is

Assertion $(A)$: Fluorine has a smaller negative electron gain enthalpy than chlorine.
Reason $(R)$: The electron-electron repulsion is higher in chlorine than in fluorine.

If the electron affinity of an element $M$ is $x \ kJ/mol$,then the ionisation potential of this element is:

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