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Ivenika [448]
3 years ago
6

Which gas law describes the relationship between volume and pressure at a constant temperature?

Chemistry
1 answer:
olasank [31]3 years ago
5 0
Boyle law is a gas law stating the pressure and the volume of a gas have an inverse relationship when held at constant temperature.

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Mariulka [41]

Answer:

matter can either be created nor destroyed but can be transmitted fromone state to another state

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3 years ago
Select all that apply. Catalysts can save money by essentially lowering the:
k0ka [10]

Answer: Options (a) and (d) are the correct answer.

Explanation:

A catalyst is the substance which helps in increasing the rate of reaction.

Activation energy is the minimum amount of energy required by reactants to start the reaction. On addition of catalyst, the path of reaction changes because the energy barrier gap reduces and hence, the activation energy also decreases.

In the absence of catalyst, we need to increase the temperature so that reaction can occur quickly.

Whereas on addition of catalyst, there is no need to increase the temperature as the catalyst itself is sufficient to increase the rate of reaction. As a result, temperature should be lowered when there is addition of catalyst in the reaction.

Thus, we can conclude that catalysts can save money by essentially lowering the activation energy and temperature required.


4 0
3 years ago
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enyata [817]

Answer:

b)5l x 10kg  c)10kg + 9l   (Not sure for the last 1)

6 0
3 years ago
How much heat is released when 15.7g of methane (c2h6) is combusted if the enthalpy of the reaction is - 1560.7 kj
lyudmila [28]

- 407.4 kJ of heat is released.

<u>Explanation:</u>

We have to write the balanced equation as,

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Here 2 moles of ethane reacts in this reaction.

Now we have to find out the amount of ethane reacted using its given mass and molar mass as,

2 mol C₂H₆ × 30.07 g of C₂H₆ / 1 mol C₂H₆ = 60.14 g of C₂H₆

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When the moon moves directly between the sun and Earth and casts its shadow over part of Earth, you are
chubhunter [2.5K]

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3 years ago
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