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DochEvi [55]
3 years ago
9

A sample of chlorine gas starting at 686 mm Hg is placed under a pressure of 991 mm Hg and reduced to a volume of 507.6 mL. What

was the initial volume of the chlorine gas container if the process was performed at constant temperature
Chemistry
1 answer:
Leviafan [203]3 years ago
3 0

Answer:

The initial volume of the chlorine gas V1=733.28mL

Explanation:

Given:

P1= 686mmHg

P2= 991mmHg

V2= 5076mL

V1=?

According to Boyle's law which states that at a constant temperature, the pressure on a gas increases as it's volume decreases.

It can be expressed as : P1V1 = P2V2

Where P1 is the initial pressure

P2= final pressure

V1= initial volume

V2 = final volume

V1= (P2V2)/P1

V1= (991mmHg*507.6mL)/686mmHg

V1=503031.6/686

V1=733.28mL

Therefore, The initial volume of the chlorine gas V1=733.28mL

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Explanation:

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ViT2 = V2T, V = V2
shusha [124]

Answer:

V₂ = 285 mL

Explanation:

Given data:

Initial volume of bag = 250 mL

Initial temperature = 19.0°C

Final temperature = 60.0°C

Final volume = ?

Solution:

The given problem will be solved by using Charles Law,

This law stated that " The volume of given amount of gas at constant pressure and constant number of moles is directly proportional to its temperature"

Mathematical relationship:

V₁/T₁  = V₂/T₂

Now we will convert the temperature into kelvin.

Initial temperature = 19.0 + 273 = 292K

Final temperature = 60.0 + 273 = 333K

Now we will put the values in formula:

V₁/T₁  = V₂/T₂

250 mL / 292K  =  V₂/ 333K

0.856 mL /K = V₂/ 333K

V₂ = 0.86×333K. mL /K

V₂ = 285 mL

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Anna007 [38]
The metric system of units is known as the International System of Units (ISU).
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