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dezoksy [38]
2 years ago
7

Write the balanced molecular chemical equation for the reaction in aqueous solution for ammonium sulfate and iron(II) chloride.

If no reaction occurs, simply write only NR. ☐⁴⁻ ☐³⁻ ☐²⁻ ☐⁻ ☐⁺ ☐²⁺ ☐³⁺ ☐⁴⁺ 1 2 3 4 5 6 7 8 9 0 ☐₁ ☐₂ ☐₃ ☐₄ ☐₅ ☐₆ ☐₇ ☐₈ ☐₉ ☐₀ + ( ) → ⇌ (s) (l) (g) (aq) Ir N Fe O Am Cl NR S H Ch Reset
Chemistry
1 answer:
dusya [7]2 years ago
7 0

The balanced molecular chemical equation for the reaction is (NH4)2SO4(aq) + FeCl2(aq) -------> FeSO4(aq) + 2NH4Cl(aq).

The rule for writing a balanced chemical reaction equation is that the number of atom of each element on the right hand side must be the same as the number of atoms of the same element on the left hand side of the reaction equation. This is achieved by performing an atom count.

The balanced molecular chemical equation for the reaction in aqueous solution for ammonium sulfate and iron(II) chloride is;

(NH4)2SO4(aq) + FeCl2(aq) -------> FeSO4(aq) + 2NH4Cl(aq)

Learn more: brainly.com/question/6505878

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Answer:

The volume of the solution must be increased to 71.429 millimeters by adding 66.359 millimeters of solute to reduce molarity from 6.82 M to 0.49 M.

Explanation:

The molarity is a unit used for solution that is equivalent to the amount of moles of solute per unit volume of solution. That is:

M = \frac{n_{st}}{V_{sol}}

Where:

n_{st} - Amount of moles of solute, measured in moles.

V_{sol} - Volume of the solution, measured in liters.

To reduce the molarity of the solution, more millimeters of solvent should be added. Firstly, the amount of moles of acetic acid inside the 6.82 M solution needs to be determined (M_{o} = 6.82\,M and V_{sol} = 5.07\times 10^{-3}\,L):

n_{st} = M_{o}\cdot V_{sol}

n_{st} = (6.82\,M)\cdot (5.07\times 10^{-3}\,L)

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Now, the resulting volume of solution after diluting the acetic acid solution is: (M_{f} = 0.49\,M and n_{st} = 0.035\,mol):

V_{sol} = \frac{n_{st}}{M_{f}}

V_{sol} = \frac{0.035\,mol}{0.49\,M}

V_{sol} = 71.429\times 10^{-3}\,L

V_{sol} = 71.429\,mL (1 L = 1000 mL)

The amount of solvent needed to dilute the solution is:

\Delta V_{sol} = 71.429\times 10^{-3}\,L - 5.07\times 10^{-3}\,L

\Delta V_{sol} = 66.359 \times 10^{-3}\,L

\Delta V_{sol} = 66.359\,mL (1 L = 1000 mL)

The volume of the solution must be increased to 71.429 millimeters by adding 66.359 millimeters of solute to reduce molarity from 6.82 M to 0.49 M.

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