Henry's law constant for `CO_2` ​ in water is `2.5×10 ^8` Pa at 298 K. Calculate milli mole of `CO_2` dissolved in 144 g water at 2.5 atm pressure at 298 K. [Take1atm=`10^5 N/m ^2`or Pa ]
A 8
B 4
C 0.8
D 0.04

henry's law constant for CO_(2) in water is 2.5xx10^(8) Pa at 298K calcualte mmole of CO_(2) dissolbed in 144 g water at 2.5 atm pressure at 298K. [take 1 atm =10^(6)(N)/(m^(2)) or Pa]

Henry's law constant for CO_(2) in water is 1.67xx10^(8) Pa at 298 K . Calculate the quantity of CO_(2) in 500mL of soda water when packed under 2.5 atm CO_(2) pressure at 298 K .

Henry's law constant for CO_(2) in water is 1.67xx10^(8) Pa at 298 K . Calculate the quantity of CO_(2) in 500mL of soda water when packed under 2.5atm CO_(2) pressure at 298 K .

Henry's law constant of CO_2 in water at 298K is 5/3K bar. IF pressure of CO_2 is 0.01 bar, find its mole fraction.

The Henry's law constant for CO_(2) in water at 298 K is 1.67 kbar. Calculate the solubility of CO_(2) at 298 K when the pressure of CO_(2) is one bar.

Henry's law constant of oxygen is 1.4 xx 10^(-3) mol "lit"^(-1) "atm"^(-1) at 298 K. How much of oxygen is dissolved in 100 mL at 298 K when the partial pressure of oxygen is 0.5 atm?

(a) Explain why on addition of 1 mole glucose to 1 litre water the boiling point of water increases . (b) Henry's law constant for CO_(2) in water is 1.67ccxx 10^(8)Pa at 298K. Calculate the number of moles of CO_(2) in 500 ml of soda water when packed under 2.53xx10^(5) Pa at same temperature.

The degree of dissociation of water is 1.8 xx10^(-9) at 298 K . Calculate the ionization constant and Ionic product of water at 298 K .

Henry's law constant for the molality of methane in benzene at 298 K is 4.27xx10^(5)mm Hg. Calculate the solubility of methane in benzene at 298 K under 760 mm Hg.

Henry's law constant for the molality of methane in benzene at 298K is 4.27xx10^(5)mm Hg . Calculate the solubility of methane in benzene at 298 K under 760 mm Hg .