Write the equilibrium expression for this reaction: (c19h8br4o5s)h– ↔ (c19h8br4o5s)2– + h+

Explanation:

The equilibrium expression for the general equilibrium represented by the equation:

is:

Then, following that sketch, you obtain:

        (C₁₉ H₈ Br₄ O₅ S) H⁻ ⇄ (C₁₉ H₈ Br₄ O₅ S)²⁻ + H⁺

         Keq = [ (C₁₉ H₈ Br₄ O₅ S)²⁻ ] [ H⁺ ] / [ (C₁₉ H₈ Br₄ O₅ S) H⁻  ]

The square brackets are used to mean molar concentration (molariy).

5.625 moles of oxygen, O₂.

Explanation:

The balanced equation for the reaction is given below:

4Al + 3O₂ —> 2Al₂O₃

From the balanced equation above,

4 moles of Al reacted with 3 moles of O₂.

Finally, we shall determine the number of mole of O₂ required to react with 7.5 moles of aluminum, Al. This can be obtained as illustrated below:

From the balanced equation above,

4 moles of Al reacted with 3 moles of O₂.

Therefore, 7.5 moles of Al will react with = (7.5 × 3)/4 = 5.625 moles of O₂.

Thus, 5.625 moles of O₂ is needed for the reaction.