Question

1. The partial pressure on the surface of Mars is 0.0070 atmospheres. The mole fractions of the top three components in the Martian atmosphere are 0.953 for CO2, 0.026 for N2, and 0.019 for Ar. In terms of torr (1 atm = 760 torr) the partial pressure of CO2 on Mars is ___________ torr, the partial pressure of N2 is ___________ torr, and the partial pressure of Ar is _____________ torr.

2. How many electrons in an atom can have the following quantum numbers: n = 4, l = 3, and m_s = +½? Enter the number as an integer.

3. Hydrogen gas (H₂) effuses 3.16 times faster than a second unknown gas. What is the molar mass of this unknown gas in g/mole?

Answer 1

question 1.)

given:

mole fraction of CO3. = 0.953

mole fraction of N2. = 0.026

mole fraction of Ar = 0.019

partial pressure on the surface of mars = 0.0070 atm or 0.0070*760 = 5.32 torr which is due to all three gases

so, P= 5.32 torr

partial pressure of CO2 = X_{​​​​​​i}. * P

where Xi is mole fraction and P is total pressure due to all three gases.

partial pressure of CO2 = 0.953*5.32 = 5.069 torr

partial pressure of N2 = 0.026* 5.32 = 0.138 torr

partial pressure of Ar = 0.019*5.32 = 0.101 torr

question 2.)

A Schrodinger wave equation gives the probability of finding particle in a 3-D space. Schrodinger wave equation have three solution so these three solution are represented by three quantum number that is

1.) principal quantum number =n

2.) azimuthal quantum number =l

3.) magnetic quantum number = m

and a 4th quantum number which tells about spin of electron that is

4.) spin quantum number = s = +1/2 or -1/2

S corresponds to only two value

whereas l = n-1

and m = -l to + l

hence

as n= 4 and l= 3 is fixed the value of m lies between -3 to +3 that is basically 7 orbital so total 14 electron

but as S is fixed that is +1/2 so only one spin is taken out of two.

so a total of of 7 electron can be represented by these given quantum number.

question 3.)

imp point = the rate of effusion of a gaseous substance is inversely proportional to square root of molar mass.

so rate of effusion of H2 is = ( 1/ 2)^ 1/2

rate of effusion of unknown gas = { (1/2) ^ 1/2 } / 3.16

so using the relationship

{ (1/2)^ 1/2 }/ 3.16=. ( 1 / M)^1/2

1/M = 1/( 2 * 3.16*3.16 )

1/M = 1/19.971

or M = 19.971 g/ mol

hence this is molar mass

hope your problem has been solved