Answer:
-162,5 kJ/mol
Explanation:
Cl(g) + 2O2(g) --> ClO(g) + O3(g) ΔH = 122.8 kJ/mol (as we used the reaction in the opposite direction, it will turn the enthalpy from exothermic to endothermic)
2O3(g) --> 3O2(g) ΔH = -285.3 kJ/mol
Cl(g) + O2(g) --> ClO(g) + O3(g) ΔH = 122.8 kJ
+ 2O3 (g) --> 3O2(g) ΔH = - 285.3 kJ
O3(g) + Cl(g) --> ClO(g) + 2O2(g) ΔH = 122.8 + (-285.3) = -162,5 kJ
Hello!
When HI is added, the buffer reacts in the following way:
1) Neutralizing of the Acid:
HI + NH₄OH → NH₄I + H₂O
2) Dissociation of the salt of a weak acid:
NH₄I → NH₄⁺(aq) + I⁻ (aq)
3) Dissociation of a weak acid to form H₃O⁺ (very little):
NH₄⁺ + H₂O ⇄ NH₃ + H₃O⁺
This series of reactions show how the adding of a strong Acid can be neutralized by the buffer, releasing instead very little amounts of Hydronium ions.
Have a nice day!
Ionic bonds involve the transfer of electrons from metal to non metal
covalent bonds involve sharing of electrons between two non metal
I took this I believe it’s A
