Magnesium oxide can be made by heating magnesium metal in the presence of oxygen gas, according to the following equation: 2 Mg(s) + O₂(g) → 2 MgO(s) When 10.1 g of magnesium (Mg) reacts with 10.5 g oxygen (O₂), 11.9 g of magnesium oxide (MgO) is formed. Determine the limiting reagent. A Determine the theoretical yield for the reaction. Report your answer with two significant figures. Do not include any units. A Determine the and percent yield for the reaction. Report your answer with two significant figures. Do not include any units.

[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant.   b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.

[References] Use the References to access important values if needed for this question. For the following reaction, 27.8 grams of sodium chloride are allowed to react with 66.9 grams of silver nitrate. sodium chloride ( aq ) + silver nitrate ( aq) → silver chloride ( s) + sodium nitrate ( aq ) What is the maximum amount of silver chloride that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams Visited Submit Answer Try Another Version 1 item attempt remaining Show Hint

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 5.4 kgkg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)