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3 years ago

Fill in the left side of this equilibrium constant equation for the reaction of nitrous acid (HNO_2) with water.

Chemistry

2 answers:

koban [17]3 years ago

6 0

Answer:

1. The equilibrium equation for the reaction between nitrous acid (HNO2) and water (H2O) is given below:

HNO2(aq) + H2O(l) <=> H3O+(aq) + NO2- (aq)

2. Ka = [H3O+] [NO2-] / [HNO2]

Explanation:

1. Step 1:

The reaction of nitrous acid HNO2 acid with water.

When nitrous acid react with water, it will produce hydronium ion (H3O+) and the corresponding nitrite ion (NO2-). This is so because an acid will dissolves in water to produce hydronium ion as the only positive ion. The equation is illustrated below:

HNO2(aq) + H2O(l) <=> H3O+(aq) + NO2- (aq)

2. Step 2:

Writing the Ka for the above equation. This is illustrated below:

The Ka is given by:

Ka = [H3O+] [NO2-] / [HNO2]

mafiozo [28]3 years ago

5 0

Answer:

$Ka=\frac{[H^+][NO_2^-]}{[HNO_2]}$

Explanation:

The reaction

The reaction of nitrous acid with water is a dissociation reaction of an acid:

$HNO_2(aq) + H_2O(l) \longrightarrow H^+(aq) + NO_2^-(aq) + H_2O(l)$

$HNO_2(aq) \longrightarrow H^+(aq) + NO_2^-(aq)$

The Ka equation

$Ka=\frac{[H^+][NO_2^-]}{[HNO_2]}$

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The given question is incomplete. The complete question is:

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Explanation:

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Answer:

ΔG = -61.5 kJ/mol (<u>Spontaneous process</u>)

Explanation:

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ΔG = ΔG° + R .T . lnQ

We don't know if the gases are at equilibrium, that's why we apply Q (reaction quotient)

ΔG = - 69 kJ/mol + 8.31x10⁻³ kJ/K.mol . 298K . ln Q

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3 years ago