Question

5. You have 100 kg of gas of the following composition: CH4 - 30% H2 - 10% N2 - 60% What is the average molecular weight of this gas?

Answer 1

Answer:

21.8 g/mol

Explanation:

Molecular weight of CH4 = 16g/mol

H2 = 2g/mol

N2 = 28g/mol

(16*30 + 2*10 + 28*60)/100

=2180/100

=21.8g/mol

Answer 2

The molar mass of the gas has been 21.8 g.

The molecular weight has been the sum of mass of each element present in the compound.

The molecular mass of the composites of gas has been:

$\rm CH_4=16\;g/mol\\H_2=2\;g/mol\\N_2=28\;g/mol$

The molecular weight of the gas has been the mass of each constituent in the sample with respect to its composition:

$\rm Mass\;of\;compound\;=\;Mass\;percent\;\times\;molar\;mass$

• Mass of methane ($M_C_H_4$) has been:

$M_C_H_4=0.30\;\times\;16\\M_C_H_4=4.8\;g$

• Mass of hydrogen ($M_H_2$) has been:

$M_H_2=0.1\;\times\;2\;g\\M_H_2=0.2\;g$

• Mass of Nitrogen ($M_N_2$) has been:

$M_N_2=0.6\;\times\;28\;g\\M_N_2=16.8\;g$

The molar mass of the gas has been the sum of the mass of all constituents. The molar mass (M) has been:

$M=M_C_H_4\;+\;M_H_2\;+\;M_N_2\\M=4.8\;+\;0.2\;+\;16.8\;g\\M=21.8\;g$

The molar mass of the gas has been 21.8 g.

For more information about the molar mass, refer to the link:

https://brainly.com/question/12127540