Name CHM 1025L: Data Sheet for Baking Soda Part A: Percent Yield of Sodium Carbonate from Baking Soda 96.438 9 Mass of test tube and beaker 98.363g Mass of test tube, beaker and baking soda (before heating) 96. 1.925 Mass of baking soda, NaHCO3 97.638 Mass of test tube, beaker and Na2CO3 residue (after heating) 1.20 Mass of sodium carbonate, Na2CO;913g-96.438a (take after heating – mass of test tube and beaker) Show the calculation for the theoretical yield of sodium carbonate below based on the starting mass of baking soda (see example 1): Mass of Na2CO3 (theoretical yield) Show the calculation for the percent yield of sodium carbonate below: Percent yield

Calculate limiting reagent and percent yield

Choose the key item that must be determined experimentally in order to calculate the percent yield as follows     Mol of product, or heat evolved, theoretical yield or

For the following reaction, 5.96 grams of iron are mixed with excess chlorine gas . The reaction yields 14.4 grams of iron(III) chloride . iron ( s ) + chlorine ( g ) iron(III) chloride ( s )   What is the theoretical yield of iron(III) chloride ?       grams What is the percent yield for this reaction ?        %

my theoretical yield was 45.0g. If my percent yield was 68.0%, how much was my actual yield?

The combustion of methane produces carbon dioxide and water. Assume that 52.8 grams of methane burned in the presence of excess oxygen gas. The percent yield is __________   percent if the reaction produces 100.9 grams of carbon dioxide.

mass of Fe: If the actual experimental yield for Fe is 8.29 g, what is the percent yield of Fe? percent yield: %

In a reaction to produce ammonia, the theoretical yield is 420.0 g. What is the percent yield if the actual yield is 224.0 g?

In a reaction where 5.0 g of aluminum reacts with 5.0 g of molecular oxygen to produce aluminum trioxide, determine the following: Limiting reactant: Theoretical yield: If your actual yield from the reaction was 25 g, what is the percent yield for the reaction?

Potassium metal reacts with oxygen gas to produce potassium oxide when heated with in air. A chemist starts a reaction with 3 moles of potassium and 5 moles of oxygen gas. What is the theoretical yield in moles of potassium oxide that can be produced? Round to 2 significant digits. If a chemist isolates 1.3 mol of potassium oxide from this reactions what is the % yield for this reaction? Round to 2 significant digits.