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MariettaO [177]
3 years ago
9

What happens to the temperature of the remaining liquid when some of the liquid evaporates

Chemistry
1 answer:
Dovator [93]3 years ago
7 0
Turns into vapor. not all of the molecules are liquid have the same energy
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Neutral atom contains 22 protons and 24 neutrons​
dezoksy [38]

Answer:

And contains 22 electrons

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2. Work is done only when an object.<br> in the<br> of the force<br> that is being applied.
sp2606 [1]

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Whenever a force is applied to an object, causing the object to move, work is done by the force. ... Work can be either positive or negative: if the force has a component in the same direction as the displacement of the object, the force is doing positive work

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Which set of procedures and observations indicates a chemical change?
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The answer is (4), (3) is merely a change in composition, thus not chemical but physical.

Answer: (4).
4 0
3 years ago
The acetylene tank contains 35.0 mol C2H2, and the oxygen tank contains 84.0 mol O2.
harkovskaia [24]

Answer:- As per the question is asked, 35.0 moles of acetylene gives 70 moles of carbon dioxide but if we solve the problem using the limiting reactant which is oxygen then 67.2 moles of carbon dioxide will form.

Solution:- The balanced equation for the combustion of acetylene is:

2C_2H_2(g)+5O_2(g)\rightarrow 4CO_2(g)+2H_2O(g)

From the balanced equation, two moles of acetylene gives four moles of carbon dioxide. Using dimensional analysis we could show the calculations for the formation of carbon dioxide by the combustion of 35.0 moles of acetylene.

35.0molC_2H_2(\frac{4molCO_2}{2molC_2H_2})

= 70molCO_2

The next part is, how we choose 35.0 moles of acetylene and not 84.0 moles of oxygen.

From balanced equation, there is 2:5 mol ratio between acetylene and oxygen. Let's calculate the moles of oxygen required to react completely with 35.0 moles of acetylene.

35.0molC_2H_2(\frac{5molO_2}{2molC_2H_2})

= 87.5molO_2

Calculations shows that 87.5 moles of oxygen are required to react completely with 35.0 moles of acetylene. Since only 84.0 moles of oxygen are available, the limiting reactant is oxygen, so 35.0 moles of acetylene will not react completely as it is excess reactant.

So, the theoretical yield should be calculated using 84.0 moles of oxygen as:

84.0molO_2(\frac{4molO_2}{5molO_2})

= 67.2molCO_2

7 0
3 years ago
Read 2 more answers
For ___, 2 lobes have positive signs while the other 2 have negative signs, showing that the opposite lobes of have same sign.​
notsponge [240]

Answer:d orbitals

Explanation: just trustme

4 0
3 years ago
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