Determine which reactant is the limiting reactant, if,
Mass of Sodium Bicarbonate= 2.00g
Mass of Citric Acid = 0.76g
Are my calculations right, or is it wrong?
(2.00g of NaHO3)(1mol/84.01g of NaHO3)(1mol of H3C6H5O7/ 3 mol of NaHO3)(192.14g of H3C6H5O7)= 1.52g of citric acid
Therefore, citric acid is limiting reactant since 0.76 g of citric acid is less than the equivalent amount which is 1.52g.
I agree.
Then, if it asks to calculate the theoretical yield of carbon dioxide based on my limiting yield,
(0.76g citric acid)(1 mol/ 192.14g citric acid)(3mol CO2/ 1mol)(44.01g CO2/1 mol)= 0.52g CO2
is that right? And if that is correct can the percent yield be over a 100% cause my percent yield came out to be 127%
* mass of carbon dioxide= 0.66g
my calculations for percent yield:
(0.66g/0.52g)(100)= 127%
Your calculations seem to be correct. To determine the limiting reactant, you need to calculate the amount of product that can be obtained from each reactant and compare them.
In this case, you have correctly converted the mass of sodium bicarbonate (NaHCO3) to moles using its molar mass (84.01g/mol). Then, you used the stoichiometric ratio between sodium bicarbonate and citric acid (H3C6H5O7) to determine the equivalent amount of citric acid. Finally, by using the molar mass of citric acid (192.14g/mol), you converted the amount back to grams.
According to your calculations, the amount of citric acid that can be obtained from 2.00g of sodium bicarbonate is 1.52g. Since the actual amount of citric acid available is 0.76g, which is less than the equivalent amount, citric acid is indeed the limiting reactant.
So, your calculations and conclusion are correct. Citric acid is the limiting reactant in this reaction.