A 5.00-L gas sample at 100.°C and 640. torr contains 20.3% neon and 79.7% xenon by mass. What are the partial pressures of the individual gases?

The answers to the question are

Partial pressure of neon = 399.42

Partial pressure of xenon = 240 torr

Explanation:

From the universal gas equation

P×V = n × R × T

n = P × V÷(R×T)

= ((640 torr /(7.5×10^(-3))× 5/ L)÷(8.314×373.15))/1000

= 0.13751 moles

Therefore, if the mass of gas = x, we have

0.203×x mass of neon and

0.797×x mass of xenon

Molar mass of neon = 20.179 g/mol

Molar mass of xenon = 131.30 g/mol

Summing the moles of neon and xenon, we have

(0.203×x)/ (20.179) + 0.797×x/( 131.30) = 0.13751 moles

1.6×10^(-2)x= 0.13751

x = 8.5306 g

Number of moles of neon =

(0.203× 8.5306 )/ (20.179) = 8.58×10(-2) moles

Mole fraction of neon = (8.58×10(-2))/ 0.13751 = 0.624

Partial pressure of neon = (mole fraction)×(total pressure of gas) = 0.624× 640 torr = 399.42 torr

Partial pressure of xenon = 240 torr

under a microscope, cancer cells may look very different from normal cells. they often have different sizes and some may be larger than normal while others are smaller. cancer cells are often abnormally shaped and the control centre of the cell (the nucleus) may have an abnormal appearance.

i think? ?