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yulyashka [42]
3 years ago
8

What particle limitation to the widespread of this reusable water bottles? Pls help someone

Chemistry
1 answer:
Sauron [17]3 years ago
3 0

Answer: Plastic water bottles

Explanation:

If you use disposable water bottles, here are some important concerns you should know about how they’re made as well as the problems they cause for the planet, your health, and your wallet.

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Neopentyl alcohol, (ch3)3cch2oh, cannot be dehydrated to an alkene without rearrangement. what is the chief product of dehydrati
emmainna [20.7K]

Dehydration is removal of water.

In alcohols dehydration is α-β elimination or 1,2 elimination, it means the hydroxyl group will be removed from α-carbon while the hydrogen will be removed from near by carbon.

In case of neopentyl alcohol there is no β hydrogen present on the β carbon [as shown in figure].

The only possible way for it to undergo dehydration is by rearrangement.

The process or mechanism can be understood as:


so the chief product is 2-methylbut-2-ene



7 0
3 years ago
In the first 85.0 s of this reaction, the concentration of no dropped from 1.12 m to 0.520 m . calculate the average rate of the
goldenfox [79]

In the first 85.0 s of this reaction, the concentration of no dropped from 1.12 m to 0.520 m .

What is rate of a reaction?

The speed at which a chemical reaction takes place is the rate of the reaction. It is the concentration change per unit time of a reactant in a reaction.

Since the concentration of NO reduces to half its initial concentration in 85 seconds that is from 1.12m to 0.520m, it can be said that 85 seconds is the half life interval for the reaction, <u>Hence on average, </u><u>half reaction</u><u> is completed in the time interval of </u><u>85 seconds</u><u>.</u>

To learn more about rate of a reaction from the given link below,

brainly.com/question/12172706

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7 0
1 year ago
What is the ideal gas law
dlinn [17]

Answer: Gases are complicated. They're full of billions and billions of energetic gas molecules that can collide and possibly interact with each other. Since it's hard to exactly describe a real gas, people created the concept of an Ideal gas as an approximation that helps us model and predict the behavior of real gases. The term ideal gas refers to a hypothetical gas composed of molecules which follow a few rules:

Ideal gas molecules do not attract or repel each other. The only interaction between ideal gas molecules would be an elastic collision upon impact with each other or an elastic collision with the walls of the container. [What is an elastic collision?]

Ideal gas molecules themselves take up no volume. The gas takes up volume since the molecules expand into a large region of space, but the Ideal gas molecules are approximated as point particles that have no volume in and of themselves.

If this sounds too ideal to be true, you're right. There are no gases that are exactly ideal, but there are plenty of gases that are close enough that the concept of an ideal gas is an extremely useful approximation for many situations. In fact, for temperatures near room temperature and pressures near atmospheric pressure, many of the gases we care about are very nearly ideal.

If the pressure of the gas is too large (e.g. hundreds of times larger than atmospheric pressure), or the temperature is too low (e.g.

−

200

C

−200 Cminus, 200, start text, space, C, end text) there can be significant deviations from the ideal gas law.

Explanation:

7 0
3 years ago
Read 2 more answers
Effects of warm tropical waters meeting with cool air.
Mars2501 [29]
A hurricane.. I believe
6 0
3 years ago
A + heat -&gt; B endothermic reaction ΔH (+)
cupoosta [38]
The best and most correct answer among the choices provided by your question is the second choice.

<span>Based on the reaction given above, as the temperature decreases, the formation of the reactants will increase.</span>


I hope my answer has come to your help. Thank you for posting your question here in Brainly. We hope to answer more of your questions and inquiries soon. Have a nice day ahead!
3 0
3 years ago
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