How To Calculate The Density Of Oxygen Gas ,O2, At 30 Deg. C And 700 MmHg
The density of hydrogen is 0,08988 g/L at 20 oC and 760 mmHg.
The density of carbon dioxide gas at -25.2 degree Celsius and 98.0 kPa is approximately 1.80 kg/m^3.
1 kiloPascal is equal to 7.5006 mmHg. So, using that conversion rate, it can be found that 769.3 mmHg is equal to 102.6 kPa.
30 degrees Celsius = 303,15 K752 mmHg = 0,9894737 atmosphere
Use the ideal gas law. PV=nRT where P=Pressure, V=Volume, n=amount (mol), R is the constant (since you have mmHg it would be 62.4) and T=temperature (convert to Kelvin). the eqation for density is mass over volume, so use the ideal gas law to solve for volume. Then calculate mass over volume.
How do you calculate the density of oxygen gas (O2) at 30 degree C. and 700 mmHg?
The volume is 0,446 L.
The density of hydrogen is 0,08988 g/L at 20 oC and 760 mmHg.
47 degrees Celsius
106.4 mmHg
500. mmHg
The density of carbon dioxide gas at -25.2 degree Celsius and 98.0 kPa is approximately 1.80 kg/m^3.
1 kiloPascal is equal to 7.5006 mmHg. So, using that conversion rate, it can be found that 769.3 mmHg is equal to 102.6 kPa.
1.79g/L ( I have the same textbook)
30 degrees Celsius = 303,15 K752 mmHg = 0,9894737 atmosphere
Use the ideal gas law. PV=nRT where P=Pressure, V=Volume, n=amount (mol), R is the constant (since you have mmHg it would be 62.4) and T=temperature (convert to Kelvin). the eqation for density is mass over volume, so use the ideal gas law to solve for volume. Then calculate mass over volume.
This is equivalent to 0.2 atm. (152 mmHg)*(1 atm)/(760 mmHg)=0.2atm