If 30cm\(^3\) of oxygen diffuses through a porous pot in 7 seconds, how long will it take 60cm\(^3\) of chlorine to diffuse through the same pot, if the vapour densities of oxygen and chlorine are 16 and 36 respectively?
According to Graham's law of diffusion of gases,the rate of diffusion of a gas is proportional to the square root of the density.
From the question, the given parameters are:
Volume of Oxygen, V\(_o\) = 30cm\(^3\), Time of diffusion of Oxygen, t\(_o\) = 7s, Vapour density of Oxygen, d\(_o\) = 16
Volume of Chlorine, V\(_c\) = 60cm\(^3\), Time of diffusion of chlorine, t\(_c\) = ?, Vapour density of Chlorine, d\(_c\) = 36
\(\frac{t_o}{t_c}\) = \(\sqrt{\frac{d_o}{d_c}}\)
\(\frac{7}{t_c}\) = \(\sqrt{\frac{16}{36}}\)
\(\frac{7}{t_c}\) = \(\frac{4}{6}\)
t\(_c\) = \(\frac{7}{4}\times {6}\)
t\(_c\) = \(\frac{21}{2}\)
Recall that the volume of Chlorine is twice that of Oxygen. Hence, t\(_c\) = 2t\(_o\)
t\(_c = 2\times \frac{21}{2}\)
t\(_c\) = 21sec - Option C
Contributions ({{ comment_count }})
Please wait...
Modal title
Report
Block User
{{ feedback_modal_data.title }}