24/7 writing help on your phone
Save to my list
Remove from my list
The purpose of this experiment was to apply stoichiometry principles to predict the amount of product formed in a precipitation reaction, accurately measure the reactants and products, determine the actual yield versus the theoretical yield, and calculate the percent yield.
Calcium chloride dihydrate (CaCl2·2H2O) was dissolved in water to create a calcium chloride solution, and stoichiometry was used to calculate the required amount of sodium carbonate (Na2CO3) for a complete reaction. The predicted and actual yield of calcium carbonate (CaCO3) precipitate were compared to calculate the percent yield.
Precipitation reactions are fundamental in chemistry, and stoichiometry plays a crucial role in predicting the quantities of reactants and products involved. In this experiment, the goal was to apply stoichiometry to forecast the amount of precipitate formed when calcium chloride dihydrate reacts with sodium carbonate. The specific objectives included:
The experiment was conducted as follows:
0 g of CaCl2·2H2O to moles yielded 0.00680 moles, and the mole ratio between CaCl2·2H2O and Na2CO3 was determined to be 1:1. Consequently, the moles of Na2CO3 were converted to grams, resulting in 0.72 g. The predicted amount of CaCO3 was calculated to be 0.68 grams.
1 g of CaCl2·2H2O was converted to moles: 0.00680 moles
Mole ratios of CaCl2·2H2O and Na2CO3: 1:1
Moles of Na2CO3 were converted to grams: 0.72 g
0.00680 moles converted to grams: 0.68 grams
Initial weight of the filter paper subtracted from final weight with precipitate: 1.9 - 1.1 = 0.8 g
Using the theoretical yield and actual yield, the percent yield was calculated: 0.8 / 0.68 = 1.176 or 117.6%
No additional questions were provided.
The experiment successfully achieved its objectives:
👋 Hi! I’m your smart assistant Amy!
Don’t know where to start? Type your requirements and I’ll connect you to an academic expert within 3 minutes.get help with your assignment