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dangina [55]
3 years ago
13

Complete the equation for the dissociation of CdCl 2 ( aq ) . CdCl2(aq). Omit water from the equation because it is understood t

o be present. equation: CdCl 2 ( aq ) ⟶
Chemistry
1 answer:
Kisachek [45]3 years ago
5 0

Answer:

The answer to your question is         CdCl₂  ⇒   Cd⁺²  +  2Cl⁻¹      

Explanation:

Data

Reactant = CdCl₂ (aq)

Process

1.- Determine the products of this reaction

The products will be the elements that form part of this compound (Cadmium and chlorine).

2.- Write the dissociation reaction

                      CdCl₂  ⇒   Cd⁺²  +  Cl⁻¹

3.- Balance the reaction

                      CdCl₂  ⇒   Cd⁺²  +  Cl⁻¹      

            Reactants    Elements     Products

                    1                 Cd                 1

                    2                 Cl                  1

The reaction is unbalanced

                     CdCl₂  ⇒   Cd⁺²  +  2Cl⁻¹      

            Reactants    Elements     Products

                    1                 Cd                 1

                    2                 Cl                  2

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The percentage yield for the reaction
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92.87 g.

Explanation:

∵ The percentage yield = (actual yield/theoretical yield)*100.

  • We need to calculate the theoretical yield:

From the balanced reaction:

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It is clear that 1 mol of PCl₃ reacts with 1 mol of Cl₂ to produce 1 mol of PCl₅.

  • We need to calculate the no. of moles of 73.7 g PCl₃:

n = mass/molar mass = (73.7 g)/(137.33 g/mol) = 0.536 mol.

<u><em>Using cross multiplication:</em></u>

1 mol of PCl₃ produce  → 1 mol of PCl₅, from stichiometry.

∴ 0.536 mol of PCl₃ produce  → 0.536 mol of PCl₅.

∴ The mass of PCl₅ (theoretical yield) = (no. of moles) * (molar mass) = (0.536 mol)*(208.24 g/mol) = 111.62 g.

<em>∵ The percentage yield = (actual yield/theoretical yield)*100.</em>

The percentage yield = 83.2%, theoretical yield = 111.62 g.

∴ The actual yield of PCl₅ = (The percentage yield)(theoretical yield)/100 = (83.2%)(111.62 g)/100 = 92.87 g.

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