Chemistry: O2 gas production

In summary, the experiment was conducted to measure the production of O2 gas. Two trials were performed, with the mass of tube and contents measured before and after O2 production. The mass of O2 generated and moles of O2 generated were also recorded, along with the temperature of H2O, barometric pressure, vapor pressure of H2O, and partial pressure of O2. Using the ideal gas relation, the volume of O2 at RT and pressure was calculated to be 70.5 mL and 77.8 mL, respectively. In order to find the volume of O2 at STP and the volume of 1 mole of O2 at STP, the ideal gas relation can be used in either of
  • #1
starry_eyes
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Data: O2 gas production
Trial 1 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 (C) 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

The items in red is what I am having problems with I figured everything else out I just need help getting started on how to find the volume of O2 at STP and the Volume of 1 mole of O2 at STP
 
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  • #2
Use the ideal gas relation in either of the following forms:

[tex]\frac {P_1V_1}{T_1} = \frac {P_2V_2}{T_2} [/tex]

OR

[tex]PV = nRT [/tex]
 
  • #3


To find the volume of O2 at STP, we can use the ideal gas law, which states that PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature. At STP (standard temperature and pressure), the temperature is 0°C or 273.15 K and the pressure is 1 atm or 760 mmHg.

First, we need to convert the given temperature of 23°C to Kelvin by adding 273.15 to get 296.15 K.

Next, we can calculate the number of moles of O2 generated in each trial by dividing the mass of O2 generated by its molar mass (32 g/mol). This gives us 0.00275 mol and 0.00255 mol for Trial 1 and Trial 2, respectively.

Now, we can plug in these values into the ideal gas law equation to solve for the volume of O2 at STP:

V = (nRT)/P

V = [(0.00275 mol)(0.0821 L atm/mol K)(296.15 K)]/ (1 atm)

V = 0.0679 L or 67.9 mL

Therefore, the volume of O2 at STP is 67.9 mL for Trial 1 and 63.2 mL for Trial 2.

To find the volume of 1 mole of O2 at STP, we can simply use the molar volume of a gas at STP, which is 22.4 L/mol. This means that at STP, 1 mole of any gas will occupy 22.4 liters of space. Therefore, the volume of 1 mole of O2 at STP is 22.4 L or 22,400 mL.
 

1. What is the chemical formula for producing O2 gas?

The chemical formula for producing O2 gas is 2H2O + 2KClO3 → 2KCl + 3O2 + 2H2O.

2. How is O2 gas produced in a laboratory setting?

O2 gas can be produced in a laboratory setting by heating a mixture of potassium chlorate (KClO3) and manganese dioxide (MnO2), which acts as a catalyst.

3. What is the purpose of producing O2 gas?

O2 gas has many important uses, such as supporting combustion, aiding in respiration for living organisms, and serving as a reactant in many industrial processes.

4. How can the production of O2 gas be measured?

The production of O2 gas can be measured using a gas syringe or a gas sensor connected to a data collection device, such as a computer or graphing calculator.

5. Are there any safety precautions that should be taken when producing O2 gas?

Yes, producing O2 gas can be dangerous and should be done with caution. It is important to wear protective gear, such as goggles and gloves, and to work in a well-ventilated area to avoid inhaling the gas. It is also important to follow proper handling and storage procedures to prevent accidents.

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