Respuesta :
Answer:
Molecules in order of decreasing rate of effusion:
[tex]^1{H}^{35}Cl>^2H^{35}Cl>^1H^{37}Cl>^2H^{37}Cl[/tex]
Explanation:
Mass of [tex]^1H^{35}Cl[/tex] gas= [tex]M_1= 36 g/mol[/tex]
Mass of [tex]^1H^{37}Cl[/tex] gas =[tex]M_2= 38 g/mol[/tex]
Mass of [tex]^2H^{35}Cl[/tex] gas =[tex]M_3= 37 g/mol[/tex]
Mass of [tex]^2H^{37}Cl[/tex] gas =[tex]M_4= 39 g/mol[/tex]
According Graham's law:
'The rate of effusion or diffusion of gas is inversely proportional to the square root of the molar mass of the gas'.The equation given by this law follows the equation:
[tex]\text{Rate of diffusion}\propto \frac{1}{\sqrt{\text{Molar mass of the gas}}}[/tex]
So, higher the molecular mass of the gas lower will be the effusion rate and vice versa.
Increasing order of molecular masses of the given gases:
[tex]M_1<M_3<M_2<M_4[/tex]
Decreasing order of effusion rate respective to gases:
[tex]R_1>R_3>R_2>R_4[/tex]
Molecules in order of decreasing rate of effusion:
[tex]^{1}\textrm{H}^{35}Cl> ^{2}\textrm{H}^{35}Cl>^{1}\textrm {H}^{37}Cl>^{2}\textrm{H}^{37}Cl[/tex]
