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3 years ago

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What is the bronsted acid of NO2- + H2O HNO2 + OH-

1 answer:

sammy [17]3 years ago

8 0

<h3><u>Answer</u>;</h3>

H2O -Bronsted Acid

<h3><u>Explanation;</u></h3>

Bronsted-Lowry acids are H+ donors , while Bronsted-Lowry bases are H+ acceptors .
A reaction of a Bronsted-Lowry acid and a Bronsted base is a neutralization reaction that is characterized by H+ transfer.

The above reaction is an example of base ionization or dissociation where;

B (aq) + H2O (l) → BH+ (aq) + OH– (aq)

That is; Base + Acid will give a conjugate acid + hydroxide ion

In our case; NO2- + H2O → HNO2 + OH- ; H2O is the H+ donor and thus, it is a Bronsted Acid.

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Answer : The mole fraction and partial pressure of $CH_4,CO_2$ and $He$ gases are, 0.267, 0.179, 0.554 and 1.54, 1.03 and 3.20 atm respectively.

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Now we have to calculate the mole fraction of $CH_4,CO_2$ and $He$ gases.

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$\text{Mole fraction of }He=\frac{\text{Moles of }He}{\text{Moles of }CH_4+\text{Moles of }CO_2+\text{Moles of }He}$

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Now we have to calculate the partial pressure of $CH_4,CO_2$ and $He$ gases.

According to the Raoult's law,

$p_i=X_i\times p_T$

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$p_T$ = total pressure of gas = 5.78 atm

$X_i$ = mole fraction of gas

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and,

$p_{He}=X_{He}\times p_T$

$p_{He}=0.554\times 5.78atm=3.20atm$

Thus, the partial pressure of $CH_4,CO_2$ and $He$ gases are, 1.54, 1.03 and 3.20 atm respectively.

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