Combining 0.353 mol Fe,0, with excess carbon produced 16.1 g Fe. Fe, O, + 3C 2 Fe +3 CO What is the actual yield of iron in moles? actual yield: mol Incorrect What is the theoretical yield of iron in moles? mol theoretical yield: Incorrect What is the percent yield?

Q: 2) from each of the possible decomposition reactions, then calculate the percent yield by dividing…

A: Theoretical yield is calculated by first writing the balanced chemical equation for the reaction .…

Q: 5. A student reacts 6.00 g of ammonium sulfide with 6.00 g of zinc (II) acetate. Upon completion of…

A: Limiting reactant :-  A reactant which is present in lesser number of molrs than required as per…

Q: 3. Magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. When 10.1 g…

A: (a) The balanced Chemical equation is - 2Mg(s) + O2(g) -----> 2MgO(s)   (b) According to the…

Q: Consider the reaction to isolate titantium metal from titanium(IV) chloride: 2 Mg(s)  +  TiCl4(l)…

A:

Q: Consider the following balanced chemical equation: 2NH3(g) + 5F2(9) 4 N2F4(9) + 6HF(g) Determine the…

A: Mass of NH3 = 78.60 g Mass of F2 = 78.60 g Known values Molar Mass of NH3 = 17 g Molar Mass of F2 =…

Q: Combining 0.251 mol Fe2O30.251 mol Fe2O3 with excess carbon produced 10.3 g Fe.10.3 g Fe.…

A: Given: 0.251 mol Fe2O3 10.3 g Fe The chemical equation involved: Fe2O3+3C⟶2Fe+3CO

Q: po Combining 0.212 mol Fe₂O3 with excess carbon produced 15.1 g Fe. Fe₂O3 + 3C 2 Fe + 3 CO What is…

A:

Q: A chemistry student prepared lead(II) iodide from 10.0 g of lead(II) nitrate and aqueous potassium…

A: Percentage yield of any compound can be obtained by dividing the obtained yield with the theoretical…

Q: When 12.4 g of CH4 is reacted with excess O2, a mass of 20.8 g of CH4O is recovered. What is the %…

A: The number of moles of a compound can be determined as: Number of moles=Given massMolar…

Q: Which substance is the limiting reactant?

A: Limiting reactant is one which consumes completely in a chemical reaction. Limiting reactant…

Q: NaCI(s) + H,SO (aq) →_ Na,so,(s) + HCI(g) - Balance the equation above. If 32.5 g NaCl and 24.5 g…

A: Balancing the equation, 2NaCI(s) + H2SO4 (aq) →_ Na2SO4(s) + 2HCI(g)  Multiply the NaCl with 2  and…

Q: When heating 16.5 g of Sb2S3 in the presence of 26 g Fe, which is the limiting reactant and which is…

A: Moles = mass / molar mass Hence moles of Sb2S3 taken = 16.5 / 338 = 0.0488  And moles of Fe = 26 /…

Q: When the equation is properly balanced, the coefficient of Fe is Fe +_ HCI →_ FeCl3 + _ H2 O 2 O 6 O…

A: On balancing , each coefficient must be whole number . It cannot be fraction. Coefficient of Fe is…

Q: Determine the limiting reactant for the reaction. O Mg(s) O 02(9) Request Answer Submit Part B…

A:

Q: Combining 0.288 mol Fe,0, with excess carbon produced 16.2 g Fe. Fe,0, +3C – 2 Fe + 3 CO What is the…

A:

Q: 64. A sample of 0.53 g of carbon dioxide was obtained by heating 1.31 g of calcium carbonate. What…

A: Given information: Actual yield of carbon dioxide = 0.53 g Mass of calcium carbonate = 1.31 g

Q: Consider the reaction. 2 Pb(s) + O2(g) → 2 PbO(s) An excess of oxygen reacts with 451.4 g of lead,…

A:

Q: Determine the percent yield for the reaction. 2Mg(s)+O2(g)→2MgO(s)2Mg(s)+O2(g)→2MgO(s) When 10.1 g…

A: Magnesium reacts with oxygen gas to form magnesium oxide. We have to find the percentage yield of…

Q: What is the percent yield?

A: Number of moles = mass/molar mass  Percent yield = (actual yield/theoretical yield) × 100%

Q: Consider the formation of lithium nitride from lithium and nitrogen: 6 Li + N2 ➜ 2 Li3N What is the…

A:

Q: A 1.274 g of copper sulfate reacts with excess zinc metal, 0.392 g copper metal was obtained…

A:

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".