The value of Henry’s law constant increases with increasing tempera

1.	The value of Henry’s law constant increases with increasing temperature?
A.	True
B.	False
Answer» B. False

Discussion

No Comment Found

Related MCQs

The atmospheric pressure is 1.0 atm and Henry’s law constant for O2 is 1.66 x 10−6 M/mm Hg at 25 °C. Assume air contains 21% oxygen. Calculate the partial pressure of oxygen. (21% of air is oxygen and the mole fraction of O2 is 0.21).
Does yeast need oxygen in fermentation process?
The value of Henry’s law constant increases with increasing temperature?
The Henry’s law constant for O2 in water at 25°C is 1.27×10−3M/atm and the mole fraction of O2 in the atmosphere is 0.21. Calculate the solubility of O2 in water at 25°C at an atmospheric pressure of 1.00 atm.Strategy: ▪ Use Dalton’s law of partial pressures to calculate the partial pressure of oxygen.▪ Use Henry’s law to calculate the solubility, expressed as the concentration of dissolved gas.
Henry Law’s Constants at a system temperature of 25°C (77°F) of nitrogen is 1600 atm/(mol/litre). Molar weight of N2 is 28.0134 g/mol and partial fraction in air is ~ 0.79. Calculate the Nitrogen dissolved in the Water at atmospheric pressure.
Henry Law’s Constants at a system temperature of 25°C (77°F) of oxygen is 756.7 atm/(mol/litre). Molar Weight of O2 is 31.9988 g/mol and partial fraction in air is ~ 0.21. Calculate the Oxygen dissolved in the Water at atmospheric pressure.
“The amount of air dissolved in a fluid is proportional to the pressure in the system”, which law is applicable to this statement?
What is the unit of oxygen solubility “C*AL”?
Does yeast need oxygen in fermentation process?$
The value of Henry‚Äö√Ñ√∂‚àö√ë‚àö¬•s law constant increases with increasing temperature?$#

The value of Henry’s law constant increases with increasing temperature?

Discussion

No Comment Found

Related MCQs

Reply to Comment