## Midterm 6A

$\Delta G^{\circ}= \Delta H^{\circ} - T \Delta S^{\circ}$

$\Delta G^{\circ}= -RT\ln K$

$\Delta G^{\circ}= \sum \Delta G_{f}^{\circ}(products) - \sum \Delta G_{f}^{\circ}(reactants)$

Siddiq 1E
Posts: 106
Joined: Fri Aug 09, 2019 12:15 am

### Midterm 6A

Hydrochloric acid is a naturally-occurring component of the gastric acid produced in
the digestive systems of most animal species, including humans. Consider this
equation for the formation of HCl:

2H2(g) + 2Cl2(g) → 4 HCl(g) ∆Ho = –92.3 kJ

(A) If the equation is reversed, the ∆Ho value equals +92.3 kJ.
(B) The four HCl bonds are stronger than the four bonds in H2 and Cl2.
(C) The ∆Ho value will be –92.3 kJ when HCl(l) is produced.
(D) 23.1 kJ of heat will be evolved when 1 mol of HCl(g) is produced.

---- How do you know that the four HCl bonds are stronger than the bonds in H2 and Cl2?

Benjamin Feng 1B
Posts: 102
Joined: Sat Sep 07, 2019 12:19 am

### Re: Midterm 6A

The stronger the bond, the more energy is needed to break them. As the reaction is exothermic, you will need to input energy to get it back to the initial state so the final products bonds are stronger and more stable.