For $Mg$,the values of $\Delta_iH_1$ and $\Delta_iH_2$ are $178 \, kcal \, mol^{-1}$ and $348 \, kcal \, mol^{-1}$ respectively. The enthalpy change for the reaction $Mg \to Mg^{2+} + 2e^-$ is ............. $kcal \, mol^{-1}$.
- A$+ 170$
- B$+ 526$
- C$- 170$
- D$- 526$
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Similar Questions
Which of the following pairs has a higher ionization enthalpy?
$(i)$ $Ne$ or $Ar$ $(ii)$ $Cl$ or $F$ $(iii)$ $F$ or $O$ $(iv)$ $N$ or $O$
$(v)$ $Na$ or $K$ $(vi)$ $Cl$ or $S$ $(vii)$ $Kr$ or $Xe$ $(viii)$ $P$ or $S$
$(i)$ $Ne$ or $Ar$ $(ii)$ $Cl$ or $F$ $(iii)$ $F$ or $O$ $(iv)$ $N$ or $O$
$(v)$ $Na$ or $K$ $(vi)$ $Cl$ or $S$ $(vii)$ $Kr$ or $Xe$ $(viii)$ $P$ or $S$
Medium
View SolutionWhich among the following elements has the highest first ionization enthalpy?
Which of the following isoelectronic ions has the lowest ionization energy?
Difficult
View SolutionMatch the following List-$I$ and List-$II$ and select the correct answer using the codes given below.
List-$I$ (Successive Ionization Enthalpy) $\left( kJ \, mol^{-1} \right)$ List-$II$
Element $IE_1$ $IE_2$ $IE_3$ Code Element $1$ $2080$ $3963$ $6130$ $(a)$ $H$ $2$ $520$ $7297$ $11810$ $(b)$ $Li$ $3$ $900$ $1758$ $14810$ $(c)$ $Be$ $4$ $800$ $2428$ $3660$ $(d)$ $B$ - - - - $(e)$ $Ne$
List-$I$ (Successive Ionization Enthalpy) $\left( kJ \, mol^{-1} \right)$ List-$II$
| Element | $IE_1$ | $IE_2$ | $IE_3$ | Code | Element |
| $1$ | $2080$ | $3963$ | $6130$ | $(a)$ | $H$ |
| $2$ | $520$ | $7297$ | $11810$ | $(b)$ | $Li$ |
| $3$ | $900$ | $1758$ | $14810$ | $(c)$ | $Be$ |
| $4$ | $800$ | $2428$ | $3660$ | $(d)$ | $B$ |
| - | - | - | - | $(e)$ | $Ne$ |
Medium
View SolutionThe $3^{rd}$ ionisation energy amongst $Li$,$Be$,$B$ and $C$ is lowest for
Medium
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