HELP An unknown gas effuses at a rate of 2.0 times the rate of CL2. What is the molar mass of the unknown gas?

Explanation:Explanation:

We can solve this equation using Graham's law of effusion:

r

1

r

2

=

√

M

M

2

M

M

1

We can substitute gas

X

and

oxygen

in for 1 and 2, respectively, to get

r

X

r

O

2

=

√

M

M

O

2

M

M

X

Since

O

2

effuses at a rate twice that of gas

X

, the ratio of the rate of effusion of

X

to

O

2

is

0.5

:

0.5

=

√

M

M

O

2

M

M

X

Since the molar mass of

O

2

is given as

32.00

g/mol

, we then have

0.5

=

√

32

l

g/mol

M

M

X

Using algebra to solve for

M

M

X

:

0.5

=

√

32

l

g/mol

√

M

M

X

√

M

M

X

=

√

32

l

g/mol

0.5

M

M

X

=

(

√

32

l

g/mol

0.5

)

2

=

128

g/mol

The molar mass of the unknown gas is thus

128

g/mol

A gas close to this value is

iodine

, with molar mass

126.90

g/mol

.

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8