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Over [174]
3 years ago
14

13. Which best describes the transition from gas to liquidy (2 points)

Chemistry
1 answer:
Vlad1618 [11]3 years ago
3 0

Energy must be removed because particles in liquid move more slowly. This statement best describes the transition from gas to liquid.

Option A

<u>Explanation:</u>

The process of transferring from gas to liquid is termed as condensation. It requires the release of energy from the gas molecules to condense them as liquid. Gas molecules inherit large amount of energy in order to move fast as the particles of gas moves faster compared to liquid.

Thus, the extra energy need to be released before converting it to liquid which has particles having less velocity of particles. So the statement describing the transition from gas to liquid is that the energy must be removed because the particles in liquid move more slowly.

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The reaction between NO2 and co to produce no and CO2 is thought to occur in two steps:
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Answer:

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Explanation:

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Why is stainless steel harder than pure iron
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What is the charge of oxygen in Na2O?
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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

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

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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