$If,{{\rm{H}}_2}\left( {\rm{g}} \right) + {\rm{C}}{{\rm{l}}_2}\left( {\rm{g}} \right) \to 2{\rm{HCl}};\Delta {H^0} = - 44{\rm{kcal}}$ 2Na(s)+2HCl(g)→2NaCl(s)+${H_2}$ (g); ∆H= -152 kcal then, ${\rm{Na}}\left( s \right) + 0.5{\rm{C}}{{\rm{l}}_2}\left( {\rm{g}} \right) \to {\rm{NaCl}}\left( s \right);\Delta {H^0} = ?$

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Application +4 | -1

If,{\mathrm{H}_2}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) \to 2\mathrm{HCl};\Delta {H^0} = - 44\mathrm{kcal}

2Na(s)+2HCl(g)→2NaCl(s)+

{H_2}

(g);
∆H= -152 kcal then,

\mathrm{Na}\left( s \right) + 0.5\mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) \to \mathrm{NaCl}\left( s \right);\Delta {H^0} = ?

View answer and explanation

Correct option: C

- 98\mathrm{kcal}

Option C (-98 kcal) is correct. By manipulating the given equations using Hess's Law, the enthalpy change for the desired reaction is calculated.