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Lyrx [107]
3 years ago
7

What pressure, in torr, would a sample of Xenon exert if it were compressed from 4001 mL to 3002 mL at constant temperature, giv

en that initially the pressure was 750.1 atm?
Chemistry
1 answer:
Andreyy893 years ago
8 0

Answer:

759779.6 torr

Explanation:

Initial volume, V₁ = 4001 mL

Final volume, V₂ = 3002 mL

Initial pressure, P₁ = 750.1 atm

We need to find the final pressure at a constant temperature. Let it be P₂. P_1V_1=P_2V_2\\\\P_2=\dfrac{P_1V_1}{V_2}\\\\P_2=\dfrac{750.1\times 4001 }{3002 }\\\\P_2=999.71\ atm

We know that,

1 atm = 760 torr

So,

999.71 atm = 759779.6 torr

Hence, there will be 759779.6 torr pressure.

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Answer:

m =\frac{p*(pi)*r^{2}*h*mw}{R*\frac{T_{1} + T_{O}}{2}}  

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The gas ideal law is  

PV= nRT (equation 1)

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n =\frac{PV}{RT}

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The cylindrical container has a constant pressure p  

The volume is the volume of a cylinder this is

V =(pi)*r^{2}*h

Where:

r = radius  

h = height  

(pi) = number pi (3.1415)

This cylinder has a radius, r and height, h so the volume is  V =(pi)*r^{2}*h

Since the temperatures has linear distribution, we can say that the temperature in the cylinder is the average between the temperature in the top and in the bottom of the cylinder. This is:  

T =\frac{T_{1} + T_{O}}{2}  

Replacing these values in the equation 2 we get:

m =\frac{P*V*mw}{R*T}   (equation 2)

m =\frac{p*(pi)*r^{2}*h*mw}{R*\frac{T_{1} + T_{O}}{2}}    

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