18.1-1. diffusion of methane through helium. a gas of ch4 and he is contained in a tube at 101.32 kpa pressure and 298 k. at one point, the partial pressure of methane is pa1 = 60.79 kpa, and at a point 0.02 m distance away, pa2 = 20.26 kpa. if the total pressure is constant throughout the tube, calculate the flux of ch4 (methane) at steady state for equimolar counterdiffusion.

5.521 × 10⁻² mol/m².s

Explanation:

Given:

Pressure of the Methane and Helium gas = 101.32 kPa

Temperature of the Methane and Helium gas = 298 K

Partial pressure of Methane,  pA₁ = 60.79 kPa

Partial pressure of Methane at point 0.02 m away,  pA₂  = 20.26 kPa

Now,

Molar flux is given as:

Here,

= 0.675 × 10⁻⁴ m²/s (for He-CH4 at 101.32 kPa and 298 K)

Z₂ - Z₁ = 0.02 m

R is the ideal gas constant = 8.314 J/mol.K

T is the temperature =  298 K

On substituting the respective values, we get

or

= 5.521 × 10⁻² mol/m².s

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.