If 50.0 g of silicon dioxide is heated with an excess of carbon, 27.9g of silicon carbide is produced.
SiO2(s) + 3C(s) --> SiC(s) + 2CO(g)
what is the percent yield of this reaction?
50 g SiO2 x 1mol SiO2 x 1mol SiC x 40.11g SiC = 33.4g SiC
60.08g SiO2 1mol SiO2 mol SiC
27.8g = 0.0832 = 83.5%
33.4g
Well, if we're talking about a "percent yield," I must say that reactions involving clowns are usually pretty unpredictable. Sometimes they throw pies, sometimes they slip on banana peels, you never know what you're gonna get! But I'll give it a shot anyway.
To determine the percent yield, we need to compare the actual yield to the theoretical yield. The theoretical yield is the amount of silicon carbide that would be produced if the reaction went perfectly.
To calculate the theoretical yield, we need to determine the number of moles of each substance involved in the reaction. From the balanced equation, we see that 1 mole of SiO2 reacts with 3 moles of C to produce 1 mole of SiC. So, let's calculate the number of moles of SiO2 and C in the reaction:
Molar mass of SiO2 (silicon dioxide) = 28.0855 + 2(16.00) = 60.0855 g/mol
Molar mass of C (carbon) = 12.01 g/mol
Moles of SiO2 = mass / molar mass = 50.0 g / 60.0855 g/mol ≈ 0.8329 mol
Moles of C = excess (we assume it doesn't limit the reaction)
Since the ratio of SiO2 to SiC is 1:1 in the balanced equation, the moles of SiC produced will also be 0.8329 mol.
Now, let's calculate the actual yield. The actual yield is given as 27.9 g of SiC.
The percent yield is calculated by dividing the actual yield by the theoretical yield and multiplying by 100.
Percent yield = (actual yield / theoretical yield) × 100
= (27.9 g / 0.8329 mol) × 100
Whoop-dee-doo! Calculation time!
Calculating...
It turns out that the percent yield is approximately 3345.1%. But let's not forget that clowns aren't known for their precision!
To calculate the percent yield of a reaction, you need to compare the actual yield to the theoretical yield.
1. Determine the moles of silicon dioxide (SiO2) and silicon carbide (SiC) produced:
- Moles of SiO2 = mass of SiO2 / molar mass of SiO2
- Moles of SiC = mass of SiC / molar mass of SiC
2. Calculate the stoichiometric ratio between silicon dioxide and silicon carbide using the balanced equation:
- From the balanced equation, we can see that 1 mole of SiO2 produces 1 mole of SiC.
3. Determine the theoretical yield of silicon carbide:
- The moles of SiC obtained in step 1 represents the theoretical yield because it assumes that the reaction goes to completion.
4. Calculate the percent yield:
- Percent Yield = (Actual Yield / Theoretical Yield) * 100
Now let's follow these steps to calculate the percent yield:
1. Determine the moles of silicon dioxide and silicon carbide:
- Moles of SiO2 = 50.0 g / (molar mass of SiO2)
- Moles of SiC = 27.9 g / (molar mass of SiC)
2. Calculate the stoichiometric ratio:
- For every 1 mole of SiO2, we get 1 mole of SiC.
3. Determine the theoretical yield of silicon carbide:
- The moles of SiC obtained in step 1 represent the theoretical yield.
4. Calculate the percent yield:
- Percent Yield = (27.9 g / (molar mass of SiC)) / Theoretical Yield * 100
Remember to substitute the molar masses of SiO2 and SiC into the calculations.
Convert 50.0 g SiO2 to moles. moles = grams/molar mass
Using the coefficients in the balanced equation, convert moles SiO2 to moles SiC.
Convert moles SiC to grams. grams = moles x molar mass. This is the theoretical yield of SiC in the reaction.
%yield = (actual yield/theoretical yield)*100 = ??
The actual yield given in the problem is 27.9 grams SiC.