441 ppb = 441 Ozone/10^9 total = partial

**pressure**O3 / p(tot) = P(O3) / 0.67**atm**3.0*10^2**atm**/ 10^9 = P(O3) p(O3) = 3.0*10^-7**atm**1 Answers · Science & Mathematics · 02/02/2014

**Standard Pressure**= 1**atm**= 760 mm Hg According to the law of partial pressures : ...1 Answers · Science & Mathematics · 02/04/2011

... for heights, forces, pressures , etc...these are called S.I. units (

**standard**international), and you'll have to use them**in**any equation you use if you're trying...2 Answers · Science & Mathematics · 31/05/2008

...temperature, he amount of dissolved gas

**in**a volume of a specified liquid id directly proportional to the partial**pressure**of the gas above the liquid.**Pressure**... units of KH =**atm**/mole fraction 0.70**atm**= 1.64 x 10^3...1 Answers · Science & Mathematics · 13/07/2017

PV=nRT, where P is

**pressure in atm**, V is volume**in**L, n is the... is just the liters per mol under**standard**conditions. So to calculate, just divide...1 Answers · Science & Mathematics · 27/02/2012

At STP (

**standard**temperature and**pressure**, 1**atm**and 273 K), an ideal gas takes up 22.4 L for each mole.**In**5.6 L of oxygen (which we assume to be an ideal gas), we have (5.6 L...1 Answers · Science & Mathematics · 09/06/2010

...partial

**pressure**CO2 + partial**pressure**air partial**pressure**air = 1**atm**...(STP) **** actually, STP is... what the US EPA uses for**standard**conditions.. see the source...regardless. ...2 Answers · Science & Mathematics · 28/10/2008

...website above. On Earth,

**standard**atmospheric**pressure**is 101.325 kPa...get the answer. (**Pressure in**atmospheres) * (Volume... = 102/101.325**atm**Volume**in**liters...1 Answers · Science & Mathematics · 29/04/2012

... left side of equation: 1. you have the

**pressure in**torr. which you need to convert to**atm**. by deviding it by 760. 2. You have the...complete. Right side: this is the**standard**, so for P, put**in**1**atm**, for T...1 Answers · Science & Mathematics · 16/10/2007

...

**pressure**" which would be 273 kelvins (**standard**temperature) and 1.0 atmosphere (**standard pressure**). R (gas constant) is 0.082 when using volume**in**liters,**pressure in atm**and T**in**kelvins. You need to change the 1.00 ton of nitrogen...1 Answers · Science & Mathematics · 30/06/2010