Question

Based on the equation 4 Ag(s) + 2 H2S(g) → 2 Ag2S(s) + 2 H2O(l), what is the mole ratio of Ag(s) to Ag2S(s)?

Answer 1

Following is the - complete Answer -&- Explanation: for the given: Question, in....typed format...

$\Rightarrow$Answer:

Molar ratio: Ag(s) : Ag2S (s) = 2 : 1 ( Answer ) ...

$\Rightarrow$Explanation:

Following is the complete Explanation, for the above Answer...

• Given:

1. chemical reaction: 4 Ag(s) + 2 H2S (g) $\rightarrow$ 2Ag2S (s) + 2 H2O (l) ------------- Equation - (1)

​​​​​​​$\Rightarrow$Where:

1. Ag(s) :   solid silver
2. H2S (g) : gaseous hydrogen sulfide.
3. Ag2S (s) : solid silver sulfide .
4. H2O (l) : liquid water.

• Step - 1:

​​​​​​​Now, the complete -and- balanced, chemical equation, for the reaction, mentioned in Equation - (1), will be the following:

$\Rightarrow$balanced reaction: 4 Ag(s) + 2 H2S (g) + O2 (g)  $\rightleftharpoons$ 2Ag2S (s) + 2 H2O (l) ---------- Equation - (2)

• Step - 2:

​​​​​​​Therefore, the following will be the desired, molar ratio, between:  Ag (s) -and- Ag2S (s)  , from the above balanced chemical equation.....i.e. from :   Equation - (2)...  [ i.e. from stoichiometry ]  

$\Rightarrow$molar ratio: Ag (s) : Ag2S = 4 : 2 = 2 : 1    ( Answer )

The above is the required molar ratio, because, as we can see above: in the balanced reaction: Equation - (2), that:  4.0 moles, of Ag(s) , reacts with H2S, and O2 , to produce:  2.0 moles, of Ag2S (s) ...

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