5. You have a 965 mL sample of methane at 92°C and a pressure of 1.29×10, tom e

Question

5. You have a 965 mL sample of methane at 92°C and a pressure of 1.29×10, tom e will the methane exert? B. Using the results from part A, if you then decrease the volume to 623 mL while keeping the temperature at - pressure will the methane exert? C. Using the results from part B, if you now increas the volume of the methane be? e the temperature to 83°C while keeping the pressure constant, what will D. If you add 1.2 moles of oxygen to the methane in part C while keeping temature and volume constant, what will partial pressure of methane, the partial pressure of oxygen, and the total pressure? E. What is the mass of the oxygen?

Explanation / Answer

A)

Consider PV= nRT

P is pressure,

v is volume ,

n is number of moles,

T is temperature,  Here T is in kelvin

R is the gas constant.

If the volume remains constant T1/P1=T2/P2

Thus (92+273)/(1.29*10^3)=(-43+273)/P2

Thus P2 is 0.81x10^3 torr

B)

Now if the temp remains constant we can use P3V3=P2V2

thus substituting values

P3x623=0.81x10^3x965

we get P3=1.26x10^3 torr

C)

Now P is constant so we use T3/V3=T4/V4

Thus (-43+273)/623= (83+273)/V4

V4=964.29 ml

If temp and volume are the same then partial pressure exerted is directly proportional to the number of moles of the gas.

D)

Calculating pressure exerted by O2 using ideal gas equation

Px0.964= 1.2x0.0821x356

P= 36.38 atm = 760x36.38 torr =27.6x10^3 torr

Total pressure is (1.26+27.6)x10^3 torr = 28.86 x10^3 torr

E)

Mass of oxygen = moles*molar mass

= 1.2x 32

= 38.4 gms

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