Calculate the number of oxygen molecules required to convert 7.50dm^3 of SO2 measured at s.t.p to SO3( molar volume of gas = 22.4dm^3, avogadros number = 6.02× 10^23)
Number of SO2 molecules in original mix = 6.02*10^23 * 7.5/22.4
need to add 1 O2 molecule for every 2 SO2 molecule so add
(6.02*10^23 * 7.5/22.4) * 0.5
Number of SO2 molecule in original mix = 6.02*1023 * 7.5/22.4. need to add 1 02 molecule for every 2 SO2 molecule so add (6.02*1023 * 7.5/22.4) * 0.5 =1.030,992 188=approximately; = 1.031.
To calculate the number of oxygen molecules required to convert 7.50 dm^3 of SO2 to SO3, we need to convert the volume of SO2 to moles and then use the stoichiometry of the balanced equation to determine the mole ratio between SO2 and O2. Finally, we can convert moles of O2 to the number of oxygen molecules.
First, we convert the volume of SO2 to moles. We can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (at standard temperature and pressure)
V = volume (in dm^3)
n = number of moles
R = ideal gas constant (0.08206 L·atm/(mol·K))
T = temperature (in Kelvin, at standard temperature and pressure stands for 273.15 K)
At standard temperature and pressure (STP), the pressure is 1 atm and the temperature is 273.15 K. Plugging these values into the equation, we get:
(1 atm) * (7.50 dm^3) = n * (0.08206 L·atm/(mol·K)) * (273.15 K)
n = (1 atm * 7.50 dm^3) / (0.08206 L·atm/(mol·K) * 273.15 K)
n ≈ 0.287 mol
Now, let's determine the mole ratio between SO2 and O2 from the balanced equation:
2 SO2 + O2 → 2 SO3
From the equation, we can see that for every 2 moles of SO2, we need 1 mole of O2.
Next, we calculate the number of moles of O2 required. Since the mole ratio is 1:1, we can simply take the same number of moles calculated for SO2.
Number of moles of O2 = 0.287 mol
Finally, we can convert the number of moles of O2 to the number of oxygen molecules by multiplying by Avogadro's number.
Number of oxygen molecules = 0.287 mol * (6.02×10^23 molecules/mol)
Number of oxygen molecules ≈ 1.73×10^23 molecules
Therefore, approximately 1.73×10^23 oxygen molecules are required to convert 7.50 dm^3 of SO2 to SO3 at STP.
To calculate the number of oxygen molecules required to convert 7.50 dm^3 of SO2 to SO3, we can follow a few steps:
Step 1: Determine the balanced chemical equation for the reaction between SO2 and O2 to form SO3. The balanced equation is:
2 SO2 + O2 → 2 SO3
This equation tells us that 2 molecules of SO2 react with 1 molecule of O2 to produce 2 molecules of SO3.
Step 2: Convert the given volume of SO2 to the number of molecules of SO2. We know that at standard temperature and pressure (s.t.p), the molar volume of any gas is 22.4 dm^3. Thus, we can use the following conversion:
7.50 dm^3 SO2 × (1 mol SO2 / 22.4 dm^3) = moles of SO2
Step 3: Once we have the number of moles of SO2, we can use the ratio from the balanced equation to find the number of moles of O2 required. The ratio tells us that for every 2 moles of SO2, we need 1 mole of O2.
moles of SO2 × (1 mol O2 / 2 mol SO2) = moles of O2
Step 4: Finally, convert the number of moles of O2 to the number of molecules of O2 using Avogadro's number (6.02×10^23 molecules/mol):
moles of O2 × (6.02×10^23 molecules/mol) = number of molecules of O2
Putting it all together with the given information:
7.50 dm^3 of SO2 becomes moles of SO2:
7.50 dm^3 SO2 × (1 mol SO2 / 22.4 dm^3) = moles of SO2
Moles of SO2 becomes moles of O2:
moles of SO2 × (1 mol O2 / 2 mol SO2) = moles of O2
Moles of O2 becomes number of molecules of O2:
moles of O2 × (6.02×10^23 molecules/mol) = number of molecules of O2
By plugging in the values and performing the calculations, you will be able to determine the number of oxygen molecules required to convert 7.50 dm^3 of SO2 to SO3.