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Gekata [30.6K]
3 years ago
15

What happens to the air particles in the bubble when you pull up on the plunger

Chemistry
1 answer:
victus00 [196]3 years ago
7 0

The air particles in the bubble are forced to expand when we pull up on the plunger.

<h3><u>Explanation:</u></h3>

Pulling creates a large amount of volume , when the volume of the air bubble is increased, air particles inside the bubble tries to accumulate all of the volume by expanding the size of the bubble. Since according to Ideal gas law,

P V = n R T

where P = Pressure of the gas

V = Volume of the gas

n = No. of moles

R = Boltzmann's constant

T = Temperature

We can observe that pressure is inversely proportional to the volume of the gas. Therefore, when we pull up the plunger, the volume of the air bubble is increased and the pressure inside it is decreased.

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In an experiment, hydrochloric acid reacted with different volumes of sodium thiosulfate in water. A yellow precipitate was form
iris [78.8K]

Answer:

I think that the trend that would be seen in the time column of the data table would be that the number of seconds would increase. I know this because for each flask, the concentration of sodium thiosulfate decreases, since less of it is being mixed with more water. Also, when the concentration of a substance decreases, then the reaction rate also decreases, as there will be fewer collisions with sulfuric acid if there are fewer moles of sodium thiosulfate. When there are fewer collisions in a reaction, the reaction itself will take longer, and so when the sodium thiosulfate is diluted, the reaction takes more time.

Explanation:

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2 years ago
Erika is asked to create a model showing a negatively charged Carbon ion. Which model should she create?
OverLord2011 [107]
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On headedama be prepared​
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Calculate the volume of hydrogen if you have 12.1 moles of Hydrogen.
vodomira [7]

To Find :

The volume of 12.1 moles hydrogen at STP.

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We know at STP, 1 mole of gas any gas occupy a volume of 22.4 L.

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The solubility of NaCH3CO2 in water is ~1.23 g/mL. What would be the best method for preparing a supersaturated NaCH3CO2 solutio
Len [333]

Answer:

b) add 130 g of NaCH₃CO₂ to 100 mL of H₂O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature.

Explanation:

The solubility of NaCH₃CO₂ in water is ~1.23 g/mL. This means that at room temperature, we can dissolve 1.23 g of solute in 1 mL of water (solvent).

<em>What would be the best method for preparing a supersaturated NaCH₃CO₂ solution?</em>

<em>a) add 130 g of NaCH₃CO₂ to 100 mL of H₂O at room temperature while stirring until all the solid dissolves.</em> NO. At room temperature, in 100 mL of H₂O can only be dissolved 123 g of solute. If we add 130 g of solute, 123 g will dissolve and the rest (7 g) will precipitate. The resulting solution will be saturated.

<em>b) add 130 g of NaCH₃CO₂ to 100 mL of H₂O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature. </em>YES. The solubility of NaCH₃CO₂ at 80 °C is ~1.50g/mL. If we add 130 g of solute at 80 °C and let it slowly cool (and without any perturbation), the resulting solution at room temperature will be supersaturated.

<em>c) add 1.23 g of NaCH₃CO₂ to 200 mL of H₂O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature.</em> NO. If we add 1.23 g of solute to 200 mL of water, the resulting solution will have a concentration of 1.23 g/200 mL = 0.00615 g/mL, which represents an unsaturated solution.

5 0
2 years ago
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