Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) A student used 117.24 g of Ag and obtained 135.49 g of AgNO3, calculate the percent yield of AgNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol

For the following reaction, 37.3 grams of sulfuric acid are allowed to react with 42.5 grams of zinc hydroxide. sulfuric acid (aq) + zinc hydroxide(s) → zinc sulfate (aq) + water (1) What is the maximum amount of zinc sulfate that can be formed? Mass= What is the formula for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? Mass= g.

39.7 mL of a 0.117 M Na2CO3 solution completely react with a 0.150 MHNO3 solution according to the following balanced chemical equation: Na2CO3(aq)+2HNO3(aq)→2NaNO3(aq)+CO2(g)+H2O(l) What mass (in grams) of carbon dioxide is formed? Express your answer with the appropriate 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.