Ca(OH)2 (s) + H₂S(g) →→→ CaS(s) + 2H₂O(1) In the reaction above, calcium hydroxide and hydrogen sulfide react to form calcium sulfide and water. If you combine 11 g of hydrogen sulfide with 15 g of calcium hydroxide: 1) Which reactant is limiting? [Select] 2) Calculate the number of moles of calcium sulfide produced if the percent yield is 100%. [Select] mol Cas

I would need help to answer the following question. In the chemical industry, determining the quantity of substances to be produced in chemical reactions is considered extremely important. The area of chemistry that determines the amount of reactants to be used and the amount of products to be obtained in chemical reactions is Stoichiometry. Considering the context above and your knowledge acquired during classes, for the reaction below calculate the amount of oxygen gas required to produce 13.5 moles of water, H2O(g), in the complete combustion of acetylene, C2H2(g)? C2H2(g) + O2(g) →  CO2(g) +  H2O(v)

Potassium chlorate, KClO 3 , decomposes upon heating in the presence of a catalyst according to the reaction below. 2KClO 3 (s) 2KCl(s)+3O 2 (g) In a certain experiment 40.0gKClO3 is heated until it completely decomposes. The experiment performed and the oxygen gas is collected and its mass is found to be 10.8g . What is the percent yield? Answer in standard notation, rounded to the nearest tenth of a percent

For the following reaction, 0.224 moles of sulfuric acid are mixed with 0.417 moles of calcium hydroxide. sulfuric acid (aq) + calcium hydroxide(s) → calcium sulfate(s) + water() What is the formula for the limiting reagent? Limiting reagent: What is the maximum amount of calcium sulfate that can be produced? Amount = moles

Please help fill out the table in the attached picture with the given information.

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:2Mg(s)+O2(g)→2MgO(s)2Mg(s)+O2(g)→2MgO(s) When 10.1 gg of Mg are allowed to react with 10.5 g of O2, 13.4 gg of MgO are collected. Determine the limiting reactant for the reaction. Express your answer as a chemical formula.

Use the References to access important values if needed for this question. For the following reaction, 4.29 grams of oxygen gas are mixed with excess propane (C3Hg). The reaction yields 2.81 grams of carbon dioxide. (1) What is the theoretical yield of carbon dioxide? (2) What is the percent yield for this reaction? C3Hg (g) +50₂ (g) 3CO₂ (g) + 4H₂O(g) % grams

Consider the following unbalanced chemical equation:  MgS (s) + O2 (g) → MgO (aq) + SO2 (g) What will be the coefficient in front of O2 in the balanced chemical equation? If there is no coefficient in front of O2 in the balanced equation,  please enter 1 as the answer.

How many grams of chlorine gas react when 266.28 grams of aluminum reacts? 2Al (s) + 3Cl2 (g) --> 2AlCl3 (s) (balanced)

When hydrogen sulfide gas is bubbled into a solution of NaOH, the reaction forms sodium sulfide and water according to the following unbalanced reaction. H₂S + 2NaOH → Na₂S + H₂O How many grams of sodium sulfide are formed if 2.75 g of hydrogen sulfide is bubbled into a solution containing 2.75 g of sodium hydroxide. (Atomic weights: Na 23.0, O 16.0, H 1.0, S 32.0)