calculate the percent yield of Cl2 in the electrolytic decomposition of hydrogen chloride if 25 g of HCl produces 13.6 of chlorine gas.
2HCl=H2+Cl2
2mol:1mol:1mol
Mole of HCl=Mass/molar mass=25/36.46=0.69mol
2/0.69=1/x x=0.345mol of Cl2
0.345*(35.45*2)=24.46gram
Percent yield=(13.6/24.46)*100%=55.60%
%yield= Practical yield/ theoretical yield
WE are calculating the theoretical yield,
2 mols of HCl gives 1mol of Cl2 Hense,
mols of HCl= 25/36.46 = 0.685 mols
mols of cl2 produced =0.685/2 = 0.342 mols
--> theoretical yeild = 0.342*70.90 = 24.30grams
Now % yield of cl2 = 13.6/24.30 = 55.96% of cl2
Well, let's break it down! The first step is to determine the molar mass of HCl, which is 36.46 g/mol. Now, we can calculate the number of moles of HCl using its molar mass:
Number of moles of HCl = Mass of HCl / Molar mass of HCl
Number of moles of HCl = 25 g / 36.46 g/mol
Number of moles of HCl = 0.686 mol
Next, we need to find the molar mass of Cl2, which is 70.906 g/mol. Since 1 mole of HCl produces 1 mole of Cl2, the number of moles of Cl2 formed will be the same as the number of moles of HCl.
Number of moles of Cl2 = 0.686 mol
Finally, we can calculate the mass of Cl2 produced using its molar mass:
Mass of Cl2 = Number of moles of Cl2 × Molar mass of Cl2
Mass of Cl2 = 0.686 mol × 70.906 g/mol
Mass of Cl2 = 48.666 g
Now, we can calculate the percent yield of Cl2:
Percent yield = (Actual yield / Theoretical yield) × 100
Percent yield = (13.6 g / 48.666 g) × 100
Percent yield = 27.92%
So, the percent yield of Cl2 in this reaction would be approximately 27.92%. Keep in mind that this calculation assumes ideal conditions and perfect experimental technique. Sometimes, in reality, we don't get the full theoretical yield due to various factors. But hey, at least there's still a decent amount of chlorine gas to entertain those swimming pool filtration systems, right?
To calculate the percent yield of Cl2 in the electrolytic decomposition of hydrogen chloride, we need to compare the actual yield (the amount of Cl2 produced) to the theoretical yield (the maximum amount of Cl2 that can be produced based on stoichiometry).
First, let's determine the balanced chemical equation for the electrolytic decomposition of hydrogen chloride:
2 HCl → H2 + Cl2
According to the balanced equation, for every 2 moles of HCl, we expect to produce 1 mole of Cl2.
Now, let's calculate the theoretical yield of Cl2 using the given amount of HCl:
molar mass of HCl = 1 g/mol + 35.5 g/mol = 36.5 g/mol
moles of HCl = 25 g / 36.5 g/mol = 0.685 moles
moles of Cl2 (theoretical) = 0.685 moles HCl / 2 moles HCl = 0.3425 moles
Now, let's calculate the actual yield of Cl2 using the given amount of chlorine gas:
molar mass of Cl2 = 35.5 g/mol + 35.5 g/mol = 71 g/mol
moles of Cl2 (actual) = 13.6 g / 71 g/mol = 0.1915 moles
Now we can calculate the percent yield by dividing the actual yield by the theoretical yield and multiplying by 100:
percent yield = (moles of Cl2 (actual) / moles of Cl2 (theoretical)) * 100
percent yield = (0.1915 moles / 0.3425 moles) * 100
percent yield = 55.98%
Therefore, the percent yield of Cl2 in the electrolytic decomposition of hydrogen chloride is approximately 55.98%.
Write the balanced equation.
2HCl ==> H2 + Cl2
Convert 25 g HCl to moles. #moles = grams/molar mass.
Using the coefficients in the balanced equation, convert moles HCl to moles Cl2.
Convert moles Cl2 to grams. # grams = moles x molar mass. This # grams is the theoretical yield.
Now calculate percent yield.
% yield = [13.6/theoretical yield]*100