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lys-0071 [83]
3 years ago
8

The chemistry teacher asked George to transfer an ideal gas from container A to container B. Container B is half the size of con

tainer A. If the temperature and moles of gas stay constant during transfer, the rate of collisions will _______________ and the pressure will __________
Chemistry
2 answers:
Rzqust [24]3 years ago
7 0
I think the answer is increase; increase

Allisa [31]3 years ago
6 0

Explanation:

According to the ideal gas equation, PV = nRT.

where,               P = pressure,                  V = volume

                         n = number of moles,     R = gas constant

                         T = temperature

Since, pressure is inversely proportional to volume. As container B is half in size as compared to container A. Therefore, pressure will increase when gas is added to container B.

Also, there will be more number of collisions between the molecules. Due to this there will be increase in rate of collisions.

Thus, we can conclude that for the given situation if the temperature and moles of gas stay constant during transfer, the rate of collisions will increase and the pressure will also increase.

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Atoms of _______ gain electrons to fill their outer electron shells and become ________ ions.
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3 years ago
Suppose 50.0g of silver nitrate is reacted with 50g of hydrochloric acid producing silver chloride and a mixture of other produc
docker41 [41]

Answer:

53.6 grams of silver chloride was produced.

Explanation:

AgNO_3+HCl+\rightarrow AgCl+HNO_3

Law of conservation of mass states that mass can neither be created nor be destroyed but it can only be transformed from one form to another form.

This also means that total mass on the reactant side must be equal to the total mass on the product side.

Mass of silver nitrate = 50.0 g

Mass of hydrogen chloride = 50.0 g

Mass of silver chloride = x

Mass of  nitric acid = 46.4 g

Mass of silver nitrate + Mass of hydrogen chloride =

                             Mass of silver chloride + Mass of  nitric acid

[te]50.0 g+50.0 g=x+46.4 g[/tex]

x=50.0 g+50.0 g - 46.4 g = 53.6 g

53.6 grams of silver chloride was produced.

8 0
3 years ago
Ammonia can be produced in the laboratory by heating ammonium chloride
AnnyKZ [126]

Answer:

Mass = 2.89 g

Explanation:

Given data:

Mass of NH₄Cl = 8.939 g

Mass of Ca(OH)₂ = 7.48 g

Mass of ammonia produced = ?

Solution:

2NH₄Cl   +  Ca(OH)₂     →    CaCl₂ + 2NH₃ + 2H₂O

Number of moles of NH₄Cl:

Number of moles = mass/molar mass

Number of moles = 8.939 g / 53.5 g/mol

Number of moles = 0.17 mol

Number of moles of Ca(OH)₂ :

Number of moles = mass/molar mass

Number of moles = 7.48 g / 74.1 g/mol

Number of moles = 0.10 mol

Now we will compare the moles of ammonia with both reactant.

                      NH₄Cl          :          NH₃

                          2              :           2

                         0.17          :          0.17

                   Ca(OH)₂         :          NH₃

                        1                :           2

                    0.10              :          2/1×0.10 = 0.2 mol

Less number of moles of ammonia are produced by ammonium chloride it will act as limiting reactant.

Mass of ammonia:

Mass = number of moles × molar mass

Mass = 0.17 mol × 17 g/mol

Mass = 2.89 g

6 0
2 years ago
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