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3 years ago

Calculate the formula mass for the compound nitrous acid.

Chemistry

1 answer:

kari74 [83]3 years ago

8 0

Answer:

47.01g/mol

Explanation:

The formula of Nitrous acid is HNO₂:

The formula mass of a compound gives the sum of the atomic masses of the elements that makes up a compound.

Atomic mass of H = 1.0079g/mol

N = 14.0067g/mol

O = 15.9994g/mol

Formula mass of HNO₂ = 1.0079 + 14.0067 + 2(15.9994)

= 1.0079 + 14.0067 +31.9988

= 47.01g/mol

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Identify the catalyst in this reaction, explain how

telo118 [61]

Question:

Sulfuric acid was once produced through the reaction of sulfur trioxide with water. Sulfur trioxide can form through the reaction of sulfur dioxide and oxygen gas. When nitrogen monoxide gas is added to the system, the reaction speeds up significantly because it proceeds through the following steps:

equations

Identify the catalyst in this reaction, explain how you know it is the catalyst, and describe how it increases the rate of the reaction.

Answer:

It is present but not consumed

NO Lowers the activation energy of the reaction

Explanation:

A catalyst is a substance that is present in a chemical reaction and enables the reaction to occur at a faster rte but does not take part n the reaction

Therefore, whereby NO is not consumed, it is the catalyst

It functions by lowering the activation energy

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3 years ago

This characteristic of hydrogen and oxygen make the water molecule polar: ______.

Finger [1]

Answer:

thé answer is b ) electronegativity

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3 years ago

In the reaction N2O4(g) 2NO2(g), what changes in color would you expect as pressure is increased at constant temperature?

skelet666 [1.2K]

Answer:

Brown color of the solution decreases

Explanation:

$NO_2$ is brown in color whereas $N_2O_4$ is colorless.

Equilibrium reaction between $NO_2$ and $N_2O_4$ is as follows:

$2NO_2\leftrightharpoons N_2O_4$

As per the Le Chatelier's principle, if pressure of a equilibrium is increased, the equilibrium will shift in the direction having fewer no. of moles of gases.

In the given equilibrium, $NO_2$ side has more no. of moles. So on increasing pressure, equilibrium will shift towards the side of $N_2O_4$ or more formation of $N_2O_4$ will take place.

Therefore, more $NO_2$ will decompose that will decrease the brown color of the solution as $N_2O_4$ is colorless.

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3 years ago

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3 years ago

A phosphate buffer is involved in the formation of urine. The developing urine contains H2PO4 and HPO42- in the same concentrati

Katen [24]

Answer:

The ionization equation is

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Explanation:

The ionization equation is

$H_{2}PO_{4}^{-} +H_{2}O$ ⇄ $HPO_{4}^{-2} +H_{3}O^{+}$ (1)

As the Bronsted definition sais, an acid is a substance with the ability to give protons thus, H2PO4 is the acid and HPO42- is the conjugate base.

The Ka expression is the ratio between the concentration of products and reactants of the equilibrium reaction so,

$Ka = \frac{[HPO_{4}^{-2}] [H_{3}O^{+}]}{[H_{2}PO_{4}^{-}] [H_{2}O]} = 6.2x10^{-8}$

The pKa is

$-Log (Ka) = -Log (6.2x10^{-8}) = 7.2$

The pKa of H2CO3 is 6,35, thus this a stronger acid than H2PO4. The higher the pKa of an acid greater the capacity to donate protons.

In the body H2CO3 is a more optimal buffer for regulating pH due to the combination of the two acid-base equilibriums and the two pKa.

If the urine is acidified, according to Le Chatlier's Principle the equilibrium (1) moves to the left neutralizing the excess proton concentration.

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3 years ago