Consider the reaction: P4(s) + 6Cl2(g) → 4PCI3(1) Given an initial mass of 11.64 g PA, an excess of Cl2, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of PCI3 produced by the reaction.

If 6.3 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, what is the mass in kg of CO₂ that is produced?

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.

P4(s) + 6Cl2(g) → 4PCl3(l) Given an initial mass of 19.14 g P4, an excess of Cl2, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of PCl3 produced by the reaction. g

[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.

In this synthesis reaction, iron and sulfur combine to form iron(II) sulfide, FeS. The balanced chemical equation is Fe (s) + S (s) → FeS (s) When 431 g of iron reacted with sulfur, a total of 502 g of iron (II) sulfide were formed. Based on the reaction stoichiometry, 678 g of iron (II) sulfide should have been produced. What is the mass of 502 g known as? actual yield percent composition theoretical yield percent yield

Chlorine gas can be produced in the laboratory by adding concentrated hydrochloric acid, HCl, to manganese(IV) oxide according to the following reaction: MnO2 (s)   +   4 HCl (aq)   →   MnCl2 (aq)   +   2 H2O (l)   +   Cl2 (g) What mass of MnO2 is required to produce 48.4 g Cl2 by the following reaction? Be sure to enter a unit with your answer.

For the following reaction, 58.6 grams of potassium hydroxide are allowed to react with 37.9 grams of phosphoric acid potassium hydroxide ( aq ) + phosphoric acid ( aq ) potassium phosphate ( aq ) + water ( I ) What is the maximum amount of potassium phosphate 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 Submit Answer Try Another Version 3 item altempts remaining

Iron(II) sulfide reacts with hydrochloric acid according to the reaction FeS(s)+2HCl(aq)→FeCl2(aq)+H2S(s) A reaction mixture initially contains 0.218 mol FeS and 0.636 mol HCl. Once the reaction has reached completion, what amount (in moles) of the excess reactant is left?

bIron metal reacts with chlorine gas giving iron(III) chloride. The balanced chemical equation for this reaction is: 2 Fe(s) + 3 Cl₂ (g) → 2 FeCl3 (s) Beginning with 32.0 g of iron, what mass of Cl2, in grams, is required for complete reaction? Mass = g Cl₂ What mass of FeCl3 can be produced? g FeCl₂ Mass=