a.Given the equation: 2CaCO3 + 2SO2 + O2 -> 2CaSO4 + 2CO2 What is the actual yield of CO2 if 7.5 mol of O2 gives a percent yield of 80%?
b. The pollutant sulfur dioxide can be removed from the emissions of an industrial plant by the reaction with calcium carbonate and oxygen. 2CaCO3 + 2SO2 + O2 -> 2CaSO4 + 2CO2 If this reaction proceeds with a 96.8% yield, how many kilograms of calcium sulfate are formed when 5.24 kg of sulfur dioxide reacts with an excess of calcium carbonate and oxygen gas?
How much CO2 should you obtain?
That's 7.5 mol O2 x (2 mols CO2/1 mol O2) = 7.5 x 2 = 15 mols CO2 = theoretical yield
Then %yield = (Actual/theoretical)*100
80 = (Actual/15)*100
Actual = ?
a. To find the actual yield of CO2, we need to know the stoichiometry of the reaction. From the balanced equation, we can see that 2 moles of CaCO3 produce 2 moles of CO2.
From the given information, we know that 7.5 mol of O2 gives a percent yield of 80%. This means that the actual yield of CO2 would be 80% of the theoretical yield.
First, we need to find the moles of CO2 produced by 7.5 mol of O2:
Using the stoichiometry of the reaction, 2 moles of O2 produce 2 moles of CO2.
So, 7.5 mol of O2 will produce (7.5 mol O2) * (2 mol CO2/2 mol O2) = 7.5 mol CO2.
Now, we can calculate the actual yield of CO2:
Actual yield of CO2 = 80% * 7.5 mol CO2 = 0.80 * 7.5 mol CO2 = 6.0 mol CO2.
Therefore, the actual yield of CO2 is 6.0 mol.
b. From the balanced equation, we can see that 2 moles of SO2 produce 2 moles of CaSO4.
To find the mass of CaSO4 formed, we need to convert the given mass of SO2 to moles, and then use the stoichiometry to determine the moles of CaSO4, and finally convert back to mass.
Given:
Mass of SO2 = 5.24 kg
First, we need to convert the mass of SO2 to moles:
Molar mass of SO2 = 32.07 g/mol + 2 * 16 g/mol = 64.07 g/mol
Number of moles of SO2 = (5.24 kg) / (64.07 g/mol) = 0.082 mol
Using the stoichiometry of the reaction, 2 moles of SO2 produce 2 moles of CaSO4.
Therefore, 0.082 mol of SO2 will produce 0.082 mol of CaSO4.
Now, we can calculate the mass of CaSO4 formed:
Molar mass of CaSO4 = 40.08 g/mol + 32.07 g/mol + 4 * 16 g/mol = 136.14 g/mol
Mass of CaSO4 formed = (0.082 mol) * (136.14 g/mol) = 11.17 g
Therefore, 5.24 kg of sulfur dioxide will produce 11.17 g of calcium sulfate.
a. To calculate the actual yield of CO2, we first need to determine the theoretical yield of CO2 using stoichiometry.
From the balanced equation provided:
2CaCO3 + 2SO2 + O2 -> 2CaSO4 + 2CO2
We can see that the balanced ratio between O2 and CO2 is 1:2. This means that for every 1 mole of O2, we should produce 2 moles of CO2.
Given that the reaction proceeds with a percent yield of 80%, we can calculate the theoretical yield of CO2 by multiplying the stoichiometric ratio by the given amount of O2:
Theoretical yield of CO2 = 2 moles CO2/1 mole O2 * 7.5 moles O2
Now, solving for the theoretical yield:
Theoretical yield of CO2 = 15 moles CO2
Since the percent yield is given as 80%, we can calculate the actual yield of CO2 by multiplying the theoretical yield by the percent yield:
Actual yield of CO2 = 15 moles CO2 * 0.80
Hence, the actual yield of CO2 is 12 moles.
b. To calculate the number of kilograms of calcium sulfate formed, we need to use the molar mass and stoichiometry.
First, let's calculate the molar mass of sulfur dioxide (SO2):
Molar mass of S = 32.07 g/mol
Molar mass of O = 16.00 g/mol (x2 since there are 2 atoms of oxygen in SO2)
Molar mass of SO2 = 32.07 g/mol + 16.00 g/mol * 2 = 64.07 g/mol
Now, let's convert the given mass of sulfur dioxide (5.24 kg) to moles:
Moles of SO2 = 5.24 kg * (1000 g/kg) / 64.07 g/mol
Next, we can use the stoichiometric ratio from the balanced equation to find the moles of calcium sulfate (CaSO4) formed.
From the balanced equation:
2CaCO3 + 2SO2 + O2 -> 2CaSO4 + 2CO2
We can see that the balanced ratio between SO2 and CaSO4 is 2:2. This means that for every 2 moles of SO2, we should produce 2 moles of CaSO4.
Moles of CaSO4 = (Moles of SO2) / 2
Now, to convert moles of CaSO4 to kilograms:
Mass of CaSO4 = Moles of CaSO4 * Molar mass of CaSO4
Using the periodic table, we can find the molar mass of CaSO4:
Molar mass of Ca = 40.08 g/mol
Molar mass of S = 32.07 g/mol
Molar mass of O = 16.00 g/mol (x4 since there are 4 atoms of oxygen in CaSO4)
Molar mass of CaSO4 = 40.08 g/mol + 32.07 g/mol + 16 g/mol * 4 = 136.14 g/mol
Finally, we can calculate the mass of CaSO4 in kilograms:
Mass of CaSO4 = Moles of CaSO4 * Molar mass of CaSO4 / (1000 g/kg)
By plugging in the values, we can find the mass of CaSO4 formed when 5.24 kg of SO2 reacts.