It is a universal constant used for all gases
Answer: The total pressure of air in lungs of an individual is 760.28 mm Hg
Explanation:
According to Dalton's law, the total pressure is the sum of individual pressures.
Given : 
=total pressure of gases = ?
= partial pressure of oxygen = 100 mm Hg
= partial pressure of nitrogen = 573 mm Hg
= partial pressure of Carbon dioxide = 0.053 atm = 40.28 mm Hg(1 atm = 760 mmHg)
= partial pressure of water vapor = 47 torr = 47 mm Hg (1torr=1 mm Hg)
putting in the values we get:
Thus the total pressure of air in lungs of an individual is 760.28 mm Hg
First you have to moles so multiply .0483L X .55M= .026565 Multiply moles by mole ratio which is 1/2, so the moles becomes .013283 now molarity=moles/volume; divide .013283/.015L=.885533M significant figures and you final answer is 0.89M
Organic Chemistry- Substances only found in living organisms.
Physical Chemistry- Structure of physical compounds and the amount of energy they have.
Inorganic Chemistry- Study of carbon containing compounds.
Nuclear power plants produce little to no greenhouse gas.
Nuclear power plants produce a large amount of energy for a small mass of fuel.
