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2 years ago

BaCl2(aq) + Na2SO4(aq) ⇄ 2NaCl(aq) + BaSO4(s)

Chemistry

1 answer:

sp2606 [1]2 years ago

3 0

Answer:

D) The equilibrium will shift to the right and more precipitate will be formed.

Explanation:

Le Châtelier's principle states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.

For the reaction:

BaCl₂(aq) + Na₂SO₄(aq) ⇄ 2NaCl(aq) + BaSO₄(s)↓,

Adding more BaCl₂ to the system:

will increase the concentration of BaCl₂ (reactants), so the equilibrium will be shifted to the right side (products side) to suppress the effect of increasing the BaCl₂.

So, the right choice is:

D) The equilibrium will shift to the right and more precipitate will be formed.

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For the reactants,

The oxidation number of hydrogen = +1
The oxidation number of oxygen = -2
The oxidation number of arsenic = +5
The oxidation number of carbon = +3

For the products,

The oxidation number of hydrogen = +1
The oxidation number of oxygen = -2
The oxidation number of arsenic = +3
The oxidation number of carbon = +4

Here, arsenic (+5 to +3) and carbon (+3 to +4) are the only oxidation numbers changing.

Note that an increase in oxidation number means electrons are lost. Thus oxidation is occurring, and a decrease in oxidation number means electrons are being gained, and thus reduction is occurring.

Also, the compound that contains the element being oxidized is the reducing agent, and the compound that contains the element being reduced is the oxidizing agent.

So, the answers are:

name of the element oxidized: Carbon

name of the element reduced: Arsenic

formula of the oxidizing agent: $\text{H}_{3}\text{AsO}_{4}$

formula of the reducing agent: $\text{H}_{2}\text{C}_{2}\text{O}_{4}$

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