If 50.0 g of sodium bicarbonate is reacted and 11.0 g of carbon dioxide is produced, what is the percent yield of carbon dioxide?
2NaHCO3 --> Na2CO3 + CO2 + H2O
You need to find the theoretical yield to go into this equation.
%yield = (actual yield/theoretial yield) x 100
Theoretical yield can be solved using this example of a stoichiometry problem.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To calculate the percent yield of carbon dioxide in this reaction, we need to compare the actual yield (11.0 g) to the theoretical yield. The theoretical yield is the maximum amount of carbon dioxide that can be produced based on the balanced equation and the quantity of the limiting reactant.
To find the theoretical yield of carbon dioxide, we need to determine which reactant is limiting. In this case, we have 50.0 g of sodium bicarbonate (NaHCO3) as the only reactant given. To determine the moles of sodium bicarbonate, we divide the given mass by its molar mass:
Molar mass of NaHCO3:
Na = 22.99 g/mol
H = 1.01 g/mol
C = 12.01 g/mol
O = 16.00 g/mol
Adding up the molar masses:
22.99 + 1.01 + 12.01 + (3 * 16.00) = 84.01 g/mol
Moles of NaHCO3 = 50.0 g / 84.01 g/mol = 0.594 mol
According to the balanced equation, the molar ratio between NaHCO3 and CO2 is 2:1. Therefore, if 0.594 mol of NaHCO3 is completely reacted, we would expect to produce 0.594 mol of CO2.
To find the theoretical yield of CO2 in grams, we multiply the moles of CO2 by its molar mass:
Molar mass of CO2:
C = 12.01 g/mol
O = 16.00 g/mol
Adding up the molar masses:
12.01 + (2 * 16.00) = 44.01 g/mol
Theoretical yield of CO2 = 0.594 mol * 44.01 g/mol = 26.10 g
Now we can calculate the percent yield of CO2:
Percent yield = (Actual yield / Theoretical yield) * 100
Percent yield = (11.0 g / 26.10 g) * 100 = 42.12%
Therefore, the percent yield of carbon dioxide in this reaction is 42.12%.