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3 years ago

What is the total ionic equation for the following reaction?

Chemistry

2 answers:

schepotkina [342]3 years ago

5 0

Answer: Option (d) is the correct answer.

Explanation:

An equation in which electrolytes are represented in the form of ions is known as an ionic equation.

Strong electrolytes easily dissociate into their corresponding ions. Hence, they form ionic equation.

$H_{2}CrO_{4}$ is a strong acid and $Ba(OH)_{2}$ is a strong bases, therefore, both of them will dissociate into ions.

Thus, total ionic equation will be as follows.

$2H^{+} + CrO_{4}^{-} + Ba^{2+} + 2OH^{-} \rightarrow Ba^{2+} + CrO_{4}^{-} + 2H_{2}O$

maxonik [38]3 years ago

5 0

Answer:

2H+ + CrO4– + Ba2+ + 2OH– > Ba2+ + CrO4– + 2H2O

Explanation:

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IgorLugansk [536]

Answer:

The reaction is not at equilibrium and reaction must run in forward direction.

Explanation:

At the given interval, concentration of NO = $\frac{4.64\times 10^{-2}}{1}M=4.64\times 10^{-2}M$

Concentration of $Br_{2}$ = $\frac{4.56\times 10^{-2}}{1}M=4.56\times 10^{-2}M$

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Reaction quotient, $Q_{c}$ , for this reaction = $\frac{[NOBr]^{2}}{[NO]^{2}[Br_{2}]}$

species inside third bracket represents concentrations at the given interval.

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So, the reaction is not at equilibrium.

As $Q_{c}< K_{c}$ therefore reaction must run in forward direction to increase $Q_{c}$ and make it equal to $K_{c}$ .

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