When 50 g of silicon dioxide is heated with an excess of carbon, 32.2 g of silicon carbide is produced. what is the percent yield of this reaction? How many grams of CO gas are made?

96.7%

Round up. its 97%

To calculate the percent yield of the reaction, we need to compare the actual yield with the theoretical yield.

Step 1: Convert the mass of silicon dioxide (SiO2) to moles.
The molar mass of SiO2 is 60.08 g/mol.

Moles of SiO2 = mass / molar mass = 50 g / 60.08 g/mol = 0.832 mol

Step 2: Use the balanced chemical equation to determine the stoichiometry between SiO2 and SiC.

The balanced equation for the reaction is:
SiO2 + 3C → SiC + 2CO

According to the equation, 1 mole of SiO2 produces 1 mole of SiC.

Step 3: Convert the moles of SiO2 to moles of SiC.
Moles of SiC = 0.832 mol

Step 4: Calculate the theoretical yield of SiC.
The molar mass of SiC is 40.10 g/mol.

Theoretical yield of SiC = moles of SiC x molar mass of SiC
Theoretical yield of SiC = 0.832 mol x 40.10 g/mol = 33.334 g

Step 5: Calculate the percent yield.
Percent yield = (actual yield / theoretical yield) x 100

% Yield = (32.2 g / 33.334 g) x 100 = 96.57%

Therefore, the percent yield of this reaction is approximately 96.57%.

Step 6: Calculate the mass of CO gas produced.
From the balanced equation, 1 mole of SiO2 produces 2 moles of CO.

Moles of CO = 2 x moles of SiO2 = 2 x 0.832 mol = 1.664 mol

The molar mass of CO is 28.01 g/mol.

Mass of CO gas = moles of CO x molar mass of CO
Mass of CO gas = 1.664 mol x 28.01 g/mol = 46.74 g

Therefore, approximately 46.74 grams of CO gas are produced in this reaction.

To determine the percent yield of a reaction, you need to compare the actual amount of the product obtained (in this case, silicon carbide) to the theoretical amount that can be obtained based on stoichiometry.

First, let's calculate the theoretical yield of silicon carbide:

1. Write the balanced chemical equation for the reaction:
SiO2 + 3C -> SiC + 2CO

2. Calculate the molar mass of silicon carbide (SiC) and silicon dioxide (SiO2):
molar mass of SiC = 28.09 g/mol
molar mass of SiO2 = 60.08 g/mol

3. Convert the given masses to moles:
moles of SiO2 = mass of SiO2 / molar mass of SiO2
moles of SiO2 = 50 g / 60.08 g/mol ≈ 0.832 mol

4. Use stoichiometry to determine the moles of silicon carbide produced:
From the balanced equation, we know that 1 mole of SiO2 reacts to produce 1 mole of SiC.
moles of SiC = moles of SiO2 ≈ 0.832 mol

5. Calculate the mass of silicon carbide using its molar mass:
mass of SiC = moles of SiC x molar mass of SiC
mass of SiC = 0.832 mol x 28.09 g/mol ≈ 23.33 g

Now, let's calculate the percent yield:

The percent yield is given by the formula:
Percent yield = (actual yield / theoretical yield) x 100

The actual yield is given as 32.2 g of SiC, and the theoretical yield is calculated as 23.33 g of SiC.

Percent yield = (32.2 g / 23.33 g) x 100
Percent yield ≈ 138.2%

The percent yield is generally expressed as a percentage, so we can round it to 138%.

Next, to determine the grams of CO gas produced, we need to use the stoichiometry of the balanced equation:

From the balanced equation, we know that for every 1 mole of SiO2 reacted, 2 moles of CO gas are produced.

moles of CO = 2 x moles of SiO2
moles of CO = 2 x 0.832 mol ≈ 1.664 mol

Now, calculate the mass of CO gas using its molar mass:

molar mass of CO = 28.01 g/mol

mass of CO = moles of CO x molar mass of CO
mass of CO = 1.664 mol x 28.01 g/mol ≈ 46.73 g

Therefore, approximately 46.73 grams of CO gas are produced.