From the given balanced equation we have find out the amount (in gm) of Ag formed from 5.50 gm of Ag₂O.
2Ag₂O(s) → 4Ag (s) + O₂ (g)
We know, molecular mass of Ag₂O= 231.7 g/mol, and atomic mass of Ag= 107.8 g/mol. Given, mass of Ag₂O=5.50 gm. Number moles of Ag₂O=
= 0.0237 moles.
From the balanced chemical reaction we get 2 (two) moles of Ag₂O produces 4 (four) moles of Ag. So, 0.0237 moles of Ag₂O produces 
moles=0.0474 moles of Ag= 0.0474 X 107.8 g of Ag=5.11g Ag.
Therefore, 5.50 g Ag₂O produces 5.11 g of Ag as per the given balanced chemical reaction.
Answer:
Step-by-step explanation:
Data:
n = 5 mol
V = 2.5 L
Calculation:
The molar concentration of the solution is 
.
Free energy is used to determine how systems change and how much work they can produce.
If the free energy of the reactants is greater than that of the products, the entropy will increase when the reaction takes place so the reaction will tend to take place spontaneously. If the free energy of the products exceeds that of the reactants, then the reaction will not take place
The Gibb's free energy change (ΔG) is:
ΔG<0⟶ Spontaneous process
ΔG>0⟶ Non-spontaneous process
ΔG=0⟶ Equilibrium process or reversible process
Gibb's free energy is a quantity used to measure the maximum amount of work done in a thermodynamic system , when the temperature and pressure are constant .
It is a state function hence it doesn't depend on path .
ΔG = ΔH - T(ΔS)
Learn more about free energy here :
brainly.com/question/10012881
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