Balance this equation: ___Ag(s)+ ___H2S(g)+___ O2(g) arrow ___Ag2S(s)+___ H2O(I)

The balanced equation :

4Ag(s)+ 2H₂S(g)+ O₂(g) ⇒2Ag₂S(s)+ 2H₂O(I)

Given

Reaction

Ag(s)+ ___H2S(g)+___ O2(g) --> ___Ag2S(s)+___ H2O(I)

Required

Balanced equation

Solution

Give a coefficient

aAg(s)+ bH₂S(g)+ cO₂(g) ⇒Ag₂S(s)+ dH₂O(I)

Make an equation

Ag, left=a, right=2 ⇒ a=2

S, left=b, right=1 ⇒b=1

H, left=2b, right=2d ⇒2b=2d ⇒2.1=2d ⇒d=1

O, left=2c ⇒right=d ⇒2c=d ⇒2c=1 ⇒c=1/2

The equation becomes :

2Ag(s)+ H₂S(g)+ 1/2O₂(g) ⇒Ag₂S(s)+ H₂O(I) x2

4Ag(s)+ 2H₂S(g)+ O₂(g) ⇒2Ag₂S(s)+ 2H₂O(I)

a chemical reaction happens

explanation:

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm