Answer:
ΔG = -105.4 kJ/mol
The system is spontaneous as written.
Explanation:
Step 1: Determine Gibbs free energy of reaction (ΔG)
We use the following expression.
ΔG = ΔH - T × ΔS
where,
ΔG = ΔH - T × ΔS
ΔG = 120.5 kJ/mol - 298 K × 0.7582 kJ/mol.K
ΔG = -105.4 kJ/mol
Step 2: Determine the spontaneity of the system.
Since ΔG < 0, the system is spontaneous as written.
AgNO₃ and Cu(NO₃)₂ are dissolved in water
It is an exothermic reaction
The stored energy in the battery does not work anymore.
Question #1
Potasium hydroxide (known)
volume used is 25 ml
Molarity (concentration) = 0.150 M
Moles of KOH used
0.150 × 25/1000 = 0.00375 moles
Sulfuric acid (H2SO4)
volume used = 15.0 ml
unknown concentration
The equation for the reaction is
2KOH (aq)+ H2SO4(aq) = K2SO4(aq) + 2H2O(l)
Thus, the Mole ratio of KOH to H2SO4 is 2:1
Therefore, moles of H2SO4 used will be;
0.00375 × 1/2 = 0.001875 moles
Acid (sulfuric acid) concentration
0.001875 moles × 1000/15
= 0.125 M
Question #2
Hydrogen bromide (acid)
Volume used = 30 ml
Concentration is 0.250 M
Moles of HBr used;
0.25 × 30/1000
= 0.0075 moles
Sodium Hydroxide (base)
Volume used 20 ml
Concentration (unknown)
The equation for the reaction is
NaOH + HBr = NaBr + H2O
The mole ratio of NaOH : HBr is 1 : 1
Therefore, moles of NaOH used;
= 0.0075 moles
NaOH concentration will be
= 0.0075 moles × 1000/20
= 0.375 M
