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Gekata [30.6K]
3 years ago
9

A sample of gas is enclosed in a container of fixed volume. Identify which of the following statements are true. Check all that

apply.If the container is heated, the gas particles will lose kinetic energy and temperature will increase.
If the container is heated, the gas particles will lose kinetic energy and temperature will increase.
If the container is cooled, the gas particles will lose kinetic energy and temperature will decrease.
If the gas particles move more quickly, they will collide more frequently with the walls of the container and pressure will increase.
If the gas particles move more quickly, they will lose energy more rapidly and collide with the walls of the container less often, and pressure will decrease.
If the gas particles move more quickly, they will collide with the walls of the container more often and with more force, and pressure will increase.
Chemistry
2 answers:
denpristay [2]3 years ago
6 0

Explanation:

As kinetic energy is the energy obtained by an object due to its motion. And, relation between kinetic energy and temperature is as follows.

                   K.E = \frac{3}{2}kT

Hence, more is the increase in temperature more will be the kinetic energy of molecules of a substance.

Therefore, with increase in kinetic energy there will occur more number of collisions as molecules collide with a force on the walls of a container which will lead to an increase in pressure also.

And, on losing kinetic energy the molecules of the substance will come closer to each other. Therefore, a decrease in temperature of the substance will also occur.

Therefore, we can conclude that the true statements are as follows.

  • If the container is cooled, the gas particles will lose kinetic energy and temperature will decrease.
  • If the gas particles move more quickly, they will collide more frequently with the walls of the container and pressure will increase.
  • If the gas particles move more quickly, they will collide with the walls of the container more often and with more force, and pressure will increase.
likoan [24]3 years ago
4 0

The answers are,

<u>B. If the container is cooled, the gas particles will lose kinetic energy and temperature will decrease.</u>

<u>C. If the gas particles move more quickly, they will collide more frequently with the walls of the container and pressure will increase.</u>

<u>E. If the gas particles move more quickly, they will collide with the walls of the container more often and with more force, and pressure will increase.</u>

Please rate <u>Brainliest</u>  (:


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A student is asked to determine the molarity of a strong base by titrating it with 0.250 M solution of H2SO4. The students is in
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Answer:

The molarity of the strong base is 0.625 M

Which procedural error will result in a strong base molarity that is too high?

⇒ Using a buret with a tip filled with air rather than the H2SO4 solution

Explanation:

<u>Step 1:</u> Data given

Molarity of H2SO4 = 0.250 M

The initial buret reading is 5.00 mL

The final reading is 30.00 mL

<u />

<u>Step 2:</u> Calculate volume of H2SO4 used

30.00 mL - 5.00 mL = 25.00 mL

<u>Step 3:</u> Calculate moles of H2SO4

0.250 M = 0.250 mol/L

Since there are 2 H+ ions per H2SO4

0.250 mol/L  * 2 = 0.500 mol/L

The number of moles H2SO4 = 0.500 mol/L * 0.025 L

Number of moles H2SO4 = 0.0125 mol

<u>Step 4</u>: Calculate moles of OH-

For 1 mol H2SO4, we need 1 mol of OH-

For 0.0125 mol of H2SO4, we have 0.0125 mol of OH-

<u>Step 5</u>: Calculate the molarity of the strong base

Molarity = moles / volume

Molarity OH- = 0.0125 mol / 0.02 L

Molarity OH - = 0.625 M

Which procedural error will result in a strong base molarity that is too high?

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Answer:

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