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adoni [48]
3 years ago
9

What happens to the average kinetic energy of the molecules of a warm substance when the temperature of the substance is slightl

y decreased? (5 points) Group of answer choices It increases. It decreases. It becomes zero. It remains unchanged.
Chemistry
2 answers:
iris [78.8K]3 years ago
5 0

Answer: Option (b) is the correct answer.

Explanation:

Average kinetic energy is defined as half of mass of gas times the square of root mean square velocity.

Mathematically,    Average K.E = \frac{1}{2}mv^{2}_{rms}

Also,   Kinetic energy = \frac{3}{2}kT

So, when there is increase in temperature then there will be increase in movement of the molecules. As a result, kinetic energy will also increase. Since, kinetic energy is proportional to temperature.

Therefore, with decrease in temperature there will be decrease in average kinetic energy of the molecules.

Thus, we can conclude that the average kinetic energy of the molecules of a warm substance also decreases when the temperature of the substance is slightly decreased.

Ber [7]3 years ago
3 0

Answer:

decreases

Explanation:

the particles have less kinetic energy as the thermal heat is decreased

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For the generic equilibrium HA(aq) ⇌ H+(aq) + A−(aq), which of these statements is true? For the generic equilibrium , which of
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<u>Answer:</u> The correct statement is if you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase.

<u>Explanation:</u>

Common ion effect is defined as the effect which occurs on equilibrium when a common ion (an ion which is already present in the solution) is added to a solution. This effect generally decreases the solubility of a solute.

Equilibrium reaction of HA and KA follows the equation:

HA\rightleftharpoons H^{+}(aq.)+A^{-}(aq.)

KA\rightleftharpoons K^+(aq.)+A^{-}(aq.)

According to Le-Chateliers principle, if there is any change in the variables of the reaction, the equilibrium will shift in the direction in order to minimize the effect.

In the equilibrium reactions, A^- ion is getting increased on the product side, so the equilibrium will shift in the direction to minimize this effect, which is in the direction of HA.

Thus, the addition of KA will shift the equilibrium in the left direction.

Equilibrium constant depends on the temperature of the system. It does not have any effect on any change of pH.

pH is defined as the negative logarithm of hydrogen ions present in the solution

  • If the solution has high hydrogen ion concentration, then the pH will be low.
  • If the solution has low hydrogen ion concentration, then the pH will be high.

As, the equilibrium is shifting in the left direction, that means concentration of H^+ ions are getting decreases. This will increase the pH of the solution.

Hence, the correct statement is if you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase.

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Answer:

c

Explanation:

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Consider the formation of the three solutionsshown in the table.
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The teacher said the volume of the liquid was 500 mL when measured a student found it was 499.7 mL what is the students percent
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Answer:

<h2>0.06 % </h2>

Explanation:

The percentage error of a certain measurement can be found by using the formula

P(\%) =  \frac{error}{actual \:  \: number}  \times 100\% \\

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error = 500 - 499.7 = 0.3

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<h3>0.06 % </h3>

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