What is the percent yield for a reaction when 166.3 grams of W2O3 combines with Carbon Monoxide but only produces 147.8 grams of W? chemical equation is W2O3+3CO------>2W+3CO2

You must first determine the theoretical yield.

mols W2O3 = grams/molar mass = ?
Use the coefficients to convert mols W2O3 to mols W.
Convert mols W grams. g = mols x atomic mass. This is the theoretical yield (TY). The actual yield in the problem is 147.8g (AY).
%W = (AY/TY)*100 = ?

To calculate the percent yield for a reaction, you need to compare the actual yield (the amount of product obtained experimentally) to the theoretical yield (the maximum amount of product that can be obtained from the given reactants).

In this case, the balanced chemical equation is:

W2O3 + 3CO --> 2W + 3CO2

First, calculate the molar mass of W2O3 (tungsten(III) oxide) and W (tungsten):

Molar mass of W2O3 = 2(W) + 3(O) = 2(183.84 g/mol) + 3(16.00 g/mol) = 399.68 g/mol
Molar mass of W = 183.84 g/mol

Next, convert the given masses of reactants to moles:

Moles of W2O3 = 166.3 g / 399.68 g/mol = 0.4161 mol
Moles of CO = 0.4161 mol (using the stoichiometric ratio from the balanced equation)

According to the stoichiometry, the theoretical yield of W (tungsten) should be equal to the moles of W2O3 used in the reaction.

The molar mass of W (tungsten) is 183.84 g/mol. Therefore, the theoretical yield of W is:

Theoretical yield of W = 0.4161 mol × 183.84 g/mol = 76.29 g

Finally, calculate the percent yield using the actual yield and theoretical yield:

Percent yield = (Actual yield / Theoretical yield) × 100
Percent yield = (147.8 g / 76.29 g) × 100 = 193.7%

Therefore, the percent yield of the reaction is approximately 193.7%.

To calculate the percent yield for a chemical reaction, you need to compare the actual yield (the amount of product obtained from the reaction) with the theoretical yield (the amount of product that should have been obtained according to the balanced chemical equation).

In this case, the balanced chemical equation is:

W2O3 + 3CO → 2W + 3CO2

First, you need to determine the theoretical yield of W (tW). This can be done using stoichiometry and the molar masses of W2O3 and W.

1) Convert the given mass of W2O3 (166.3 grams) to moles:
moles of W2O3 = mass / molar mass
moles of W2O3 = 166.3 g / (2 * atomic mass of W + 3 * atomic mass of O)

You can find the molar masses of elements from the periodic table.

2) Use the stoichiometry of the balanced equation to determine the moles of W produced (moles of W):
moles of W = 2 * moles of W2O3

3) Convert the moles of W to the mass of W (tW):
tW = moles of W * atomic mass of W

Now that you have the theoretical yield (tW), you can calculate the percent yield using the given actual yield (147.8 grams of W):

Percent yield = (actual yield / theoretical yield) * 100%
Percent yield = (147.8 g / tW) * 100%

Plug in the calculated values for tW and solve for the percent yield.