Four Aluminum atoms combine with three chlorine molecules to produce solid aluminum chloride. Balanced reaction is: 2AI + 3CI2 2AICI3 Use this particulate representations of the reaction to determine the limiting and excess reactant. Key = aluminum = chlorine Before reaction After reaction

80°F Mostly sunny Stoichiometry can be used to determine the mass (in grams) of a product. O True O False Search H &

A grease fire started on the stove, it was then covered completely with a fire blanket so that the fire goes out. Identify the limiting reactant in this situation

How many grams of N2 are needed to completely (stoichiometrically) react with 222 g of Br2 ? N2 + 3 Br2 2 NB13 + 44.0 kJ The molar mass of Br2 is g and the molar mass of N2 is mol Br2 (2.22 x 102 g Br2)(- mol Br2 g Br2 mol N2 mol Br2 (-- -) = mol N2 mol Br2 g N2 mol N2 (-- -) = |v g N2 mol N2 а. 1 b. 2 С. 3 d. 4 е. 5 f. 253.719 g. 3.38 х 100 h. 3.26 x 103 i. 44.0 j. 1.33 x 102 k. 9.77 x 103 I. 4.44 x 102 m. 6.66 x 10² n. 500.0 o. 556 р. 90.0 q. 3.2852 r. 159.81 s. 28.013 t. 1.750 u. 0.8750 v. 13.0 w. 0.46306 х. 1.3892 у. 24.5 z. 38.5 аа. 2.190 bb. evolved Cc. absorbed dd. exothermic ee. endothermic

Use the References to access important values if needed for this question. For the following reaction, 3.56 grams of nitrogen gas are mixed with excess hydrogen gas. The reaction yields 3.75 grams of ammonia. nitrogen (g) + hydrogen (g) ammonia(g) grams What is the theoretical yield of ammonia ? What is the percent yield for this reaction ? Submit Answer 5 question attempts remaining %

For the following reaction, 6.79 grams of sulfur are mixed with excess carbon monoxide. The reaction yields 10.7 grams of sulfur dioxide. sulfur (s) + carbon monoxide →sulfur dioxide (g) + carbon (s) What is the theoretical yield of sulfur dioxide ? grams What is the percent yield of sulfur dioxide ? %

For the following reaction, 6.42 grams of oxygen gas are mixed with excess hydrogen sulfide. The reaction yields 1.97 grams of water. hydrogen sulfide (g) + oxygen water (1) sulfur dioxide (g) What is the theoretical yield of water ? | grams What is the percent yield of water ? %

B. Stoichiometry and Percent Yield DATA 1. Mass of sodium carbonate 2. Mass of filter paper 3. Mass of dry filter paper and calcium carbonate product CALCULATIONS AND QUESTIONS (show all of your work) 1. Mass of dried product (actual yield) (Mass of dry filter paper and calcium carbonate product - mass of filter paper) 1.0 g 1.2g 2.69 2. Write the balanced chemical equation for the reaction of sodium carbonate and calcium chloride. (Ignore the hydrate in this equation) 2.89 3. Use stoichiometry to calculate the theoretical yield of calcium carbonate product based on the starting mass of sodium carbonate. 4. Calculate the percent yield of the reaction based on the actual yield of dried calcium carbonate product and the theoretical yield of calcium carbonate product. 11

Consider the combustion of hydrogen to make water. If you start with 2.47 grams of H2 and 12.02 grams of O2, what is the limiting reactant and the theoretical yield of water? Limiting reactant: _____ Theoretical yield: _____

Barium chloride in solution and silver nitrate in solution react to form silver chloride and barium nitrate.-i- Write and balance the equation. -ii- Identify the type of reaction -iii How many moles of silver chloride are produced from 4.56 moles of barium chloride?