How do you find the
-Volume of O2 at STP
-Volume of 1 mole of O2 at STP
Volume of O2 can be found, if you know the parameters, by PV = nRT.
The volume of a mole of O2 at STP is 22.4 L, in fact, that's the volume of a mole of any ideal gas at STP.
You can substitute into PV = nRT and calculate 22.4 L.
Data:O2 gas production
Tria1 Trial 2
Mass of tube and contents prior to O2 production (g) 24.5196 g 24.4328 g
Mass of tube and contents after O2 production (g) 24.4315 g 24.3513 g
Mass of O2 generated (g) 0.0881 g 0.0815 g
Moles of O2 generated (mol) 0.00275 mol 0.00255 mol
Temperature of H2O („aC) 23 O C 23 O C
Barometric Pressure (mmHg) 621.5 mmHg 621.5 mmHg
Vapor Pressure of H2O (mmHg) 21.1 mm Hg 21.1 mm Hg
Partial Pressure of O2 (mmHg) 600.4 mm Hg 600.4 mm Hg
Volume of O2 at RT&Pressure 70.5 77.8
Volume of O2 at STP
Volume of 1 mole of O2 at STP
Data:O2 gas production
Tria1 Trial 2
Mass of tube and
contents prior to
O2 production (g) 24.5196 g 24.4328 g
Mass of tube and
contents after O2
production (g) 24.4315 g 24.3513 g
Mass of O2
generated (g) 0.0881 g 0.0815g
Moles of
O2 generated(mol) 0.00275 mol 0.00255
Temperature of H2O 23 O C 23 O C
Barometric
Pressure (mmHg) 621.5 mmHg 621.5
Vapor Pressure
of H2O (mmHg) 21.1 mm Hg 21.1
Partial Pressure
of O2 (mmHg) 600.4 mm Hg 600.4
Volume of O2
at RT&Pressure 70.5 77.8
Volume of O2 at STP (these I don't know )
* Volume of 1 mole of O2 at STP *
I don't know if these two latter posts are new questions or not. If so, please clarify them.
The things I posted later are all the info I have to figure out the questions I need answered ..
It still isn't clear to me. You need to be more specific.
O2 gas is produced in the lab by (ususally) heating KClO3 but heating other chlorates and nitrates will also work. For O2 commercially, it usually is done by liquifying air, then separating the components by fractional distillation.
I understand that I already did the lab... these are the results from the lab.... I did two trial I am having trouble finding the volume of O2 STP and the mole STP what do I use to figure out those volumes
To find the volume of O2 at STP (Standard Temperature and Pressure) and the volume of 1 mole of O2 at STP, we need to use the Ideal Gas Law equation: PV = nRT.
Let's break down the equation to understand the variables:
- P: Pressure (in units of pressure, such as atm or Pa)
- V: Volume (in units of volume, such as liters or m³)
- n: Number of moles of gas
- R: Ideal Gas Constant (varying depending on the units used for pressure and volume)
- T: Temperature (in units of temperature, such as kelvin)
At STP, the conditions are standardized as follows:
- Temperature (T): 273.15 K (0 °C)
- Pressure (P): 1 atm (atmosphere) or 101.325 kPa (kilopascal)
1. Volume of O2 at STP:
To find the volume of O2 gas at STP, we need to know the number of moles (n) of O2 gas.
Suppose we have the number of moles of O2 gas (n). We can rearrange the Ideal Gas Law equation as follows: V = nRT/P.
Since we want to find the volume at STP, we substitute the known values:
- T: 273.15 K
- P: 1 atm (or 101.325 kPa)
- R: Use the ideal gas constant appropriate for the units you're working with.
For example, if we are using atm as the unit for pressure and liters as the unit for volume, we use the ideal gas constant R = 0.0821 L·atm/(mol·K).
Knowing these values, plug them into the equation, along with the number of moles of O2 (n), to calculate the volume (V) of O2 at STP.
2. Volume of 1 mole of O2 at STP:
To find the volume of 1 mole of O2 gas at STP, we set the number of moles (n) to 1 in the equation: V = RT/P.
Using the same values for T and P as in the previous example, along with the ideal gas constant R, we can compute the volume (V) of 1 mole of O2 gas at STP.