Question

$\Delta G^o$ for the reaction:

$AgCl\left(s\right)+1/2H_2\left(g\right)⟶Ag\left(s\right)+H^{+}+C{l}^{-}$ is $-21.52kJ$

$\Delta G^o$ for the reaction:

$2AgCl\left(s\right)+H_2\left(g\right)\to 2Ag\left(s\right)+2H^{+}+2C{l}^{-}$ is:

• A. $-21.52KJ$
• B. $-10.76KJ$
• C. $-43.04KJ$
• D. $-45.04KJ$

Answer 1

The correct option is A $-21.52KJ$

$AgCl\left(s\right)+1/2H_2\left(g\right)\to Ag\left(s\right)+H^{+}+C{l}^{-};△G^o=-21.52kJ$

$2AgCl\left(s\right)+H_2\left(g\right)\to 2Ag\left(s\right)+2H^{+}+2C{l}^{-};△G^{\circ }=?$

$△G^{\circ }$ represents the Gibbs free energy than can be used to calculate the maximum reversible work that may be performed by a thermodynamic system at a constant temperature and pressure.

$△G^{\circ }$ doesn't depend upon moles of the reacting species and the product formed. Hence, $△G^{\circ }=-21.52KJ$ when $2$ moles of $AgCl$ reacts.