How can we figure the reactants ? For part 1 and 2 ? # Workshop 10: Stoichiometry and Limiting ReagentIn chemistry, we represent chemical reactions using balanced chemical equations. These equations represent mole ratios and can be used to perform stoichiometric calculations. The limiting reagent in a chemical reaction is the reactant that will be totally consumed when the chemical reaction is complete. The amount of product that you can form is limited by the amount of the limiting reagent that you begin with. Today you will solve a couple of old exam questions to practice stoichiometry calculations and the method of dimensional analysis.## Part I. Limiting Reagent1. **Al reacts with O₂ to produce Al₂O₃. Write and balance the chemical equation for this reaction:** Discuss the following questions among your group members: **A.** If one reacts 12 atoms of aluminum and 11 molecules of oxygen, without performing any calculations, predict which one of the reactants (if any) will still be present in the reaction mixture after the reaction is completed: do you expect to have any aluminum atoms left in the reaction mixture or any oxygen molecules? **B.** If one reacts 12 grams of aluminum and 11 grams of oxygen, without performing any calculations, predict which one of the reactants (if any) will still be present in the reaction mixture after the reaction is completed: do you expect to have any aluminum atoms left in the reaction mixture or any oxygen molecules? Write down your group’s predictions here and sign below: **A.** Some of ________________ will be present in the reaction mixture after the reaction. **B.** Some of ________________ will be present in the reaction mixture after the reaction.2. **Now let’s see if your predictions match the actual results.** **A.** Draw the maximum number of Al₂O₃ formula units that can be produced in this process. **Diagram Explanation:** - The diagram consists of rows of circles representing aluminum atoms (O) and pairs of circles representing oxygen molecules (⦁⦁). - It shows the combination of these reactants to form the product, Al₂O₃, where each formula unit consists of two aluminum atoms and three oxygen atoms. **Answer:** __________ is a limiting reactant and we will have __________ atoms/molecules of __________ left in the reaction mixture after the reaction is completed. **General Chemistry 1****B.** Calculate how many grams of aluminum oxide can be produced in a reaction involving 12.0 g of aluminum and 11.0 g of oxygen gas. How many grams of product will be made in this reaction and how many grams of excess reactant will be left after the reaction?\( MM(\text{Al}) = \_\_\_\_\_ \, \text{g/mol} \quad MM(\text{O}_2) = \_\_\_\_\_ \, \text{g/mol} \quad MM(\text{Al}_2\text{O}_3) = \_\_\_\_\_ \, \text{g/mol} \)Write down and balance the chemical reaction: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_**i. Plan for the solution:**a) Find the limiting reagent:- *Calculate the amount of aluminum oxide (in moles) that can be produced from the reaction of 12.0 g of aluminum with the excess of oxygen;*- *Calculate the amount of aluminum oxide (in moles) that can be produced from the reaction of 11.0 g of oxygen with the excess of aluminum;*b) Calculate the amount of aluminum oxide (in grams) that can be produced in this process.c) Calculate how many grams of excess reagent will be used in the process.d) Calculate how many grams of excess reagent will be left after the reaction.**ii. Solve the problem following the plan:****iii. Assess the result:** Does your answer make sense? Please provide the justification. You can do this in a few different ways. One way is to work out the units; the other way is to try to estimate the value to see if you get the correct order of magnitude.**Answer:** \_\_\_\_\_\_\_\_ is a limiting reactant. \_\_\_\_\_ grams of aluminum oxide will be produced in this reaction and we will have \_\_\_\_\_ grams of \_\_\_\_\_\_\_\_ (excess reactant) left in the reaction mixture after the reaction is completed.

The reactant which is present in lesser amount in the chemical reaction and which guides the amount…

Workshop 10: Stoichiometry and Limiting Reagent In chemistry we represent chemical reactions using balanced chemical equations. These equations represent mole ratios and can be used to perform stoichiometric calculations. The limiting reagent in a chemical reaction is the reactant that will be totally consumed when the chemical reaction is complete. The amount of product that you can form is limited by the amount of the limiting reagent that you begin with. Today you will solve a couple of old exam questions to practice stoichiometry calculations and the method of dimensional analysis. Part I. Limiting reagent. 1. Al reacts with O₂ to produce Al2O3. Write and balance the chemical equation for this reaction: Discuss the following questions among your group members: A. If one reacts 12 atoms of aluminum and 11 molecules of oxygen. Without performing any calculations predict which one of the reactants (if any) will still be present in the reaction mixture after the reaction is completed: do you expect to have any aluminum atoms left in the reaction mixture or any oxygen molecules? B. If one reacts 12 grams of aluminum and 11 grams of oxygen. Without performing any calculations predict which one of the reactants (if any) will still be present in the reaction mixture after the reaction is completed: do you expect have any aluminum atoms left in the reaction mixture or any oxygen molecules? Write down your group's predictions here and sign below: A. Some of B. Some of 2. Now let's see if your predictions match the actual results. A. Draw the maximum number of Al2O3 formula units that can be produced in this process. Products (Al2O3 = O0000) will be present in the reaction mixture after the reaction. will be present in the reaction mixture after the reaction. Reactants (O= aluminum atom, 0 = oxygen molecule) 0000 00 00 00 00 0000 000 0 Answer: + 00 00 00 00 ➜ 00 00 00- is a limiting reactant and we will have left in the reaction mixture after the reaction is completed. [Excess] atoms/molecules of