Question

Supose the gas above the soda in a bottle of soft drink is pure CO2 at a pressure of 4.5 atm. Calculate [CO2) at 25 C in mol/L at an elevation of 1100.0 m. Henry's law at 25°C is 0.03363 mol/(L*atm) A 0.151 M B 0.05 M C 0.084 M D 0.168 M E 0.118 M

Answer 1

Answer:-

Given:-

partial pressure of CO₂ gas in soft drink bottle (p_CO2 ) = 4.5 atm

Henry Law constant of CO₂ gas (K_CO2) = 0.03363 mol /L.atm

molar concentration of CO₂ gas i.e [CO₂] = ?

As we know that at an elevation of 1100.0 m , there is no change on the partial pressure of CO₂ gas because CO₂ gas is closed in the soft drink bottle. therefore according to the Henry law ' At constant temperature , the concentration of gas dissolved is directly proportional to its partial pressure'.

concentration of gas (c)   $\alpha$  partial pressure of gas (p)

so

concentration of gas (c) =  K_H$\times$ partial pressure of gas (p)

where

  K_H = Henry Law constant of gas

therefore

molar concentration of CO₂ gas i.e [CO₂] = Henry Law constant of CO₂ gas (K_CO2) $\times$ partial pressure of CO₂ gas in soft drink bottle (p_CO2 )

molar concentration of CO₂ gas i.e [CO₂] = 0.03363 mol /L.atm $\times$ 4.5 atm

molar concentration of CO₂ gas i.e [CO₂] = 0.151 mol /L

or

molar concentration of CO₂ gas i.e [CO₂] = 0.151 M (i.e the answer)

therefore correct option is 'A' i.e 0.151 M