Step 2b: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al O, from the complete reaction of 201 grams Fe,o according to the following balanced chemical equation: 2 Al(s) + Fe 0,(s)AlO,(s)+ 2 Fe(s) STARTING AMOUNT

Upon reaction of 1.27 gof copper sulfate with excess zinc metal, 0.239 g copper metal was obtained as an experimental result according to the equation: CuSOalaq) + Zn(s) Culs) + ZnSO.laq) Before the experiment was carried out the theoretical yield calculation was completed to predict the maximum amount of copper that could be isolated. The answer was 0.506 g of Cu. What is the percent yield in standard notation?

Chloroform, CHCl3, reacts with chlorine, Cl2, to form carbon tetrachloride, CCl4, and hydrogen chloride, HCl. In an experiment 25 grams of chloroform and 0.36 mol of chlorine were mixed. Which is the limiting reactant?  The equation is given as                                               CHCl3       +      Cl2         =     CCl4      +     HCl

Consider the following unbalanced chemical equation: Fe3O4 (aq) + CO (g) → CO2 (g) + Fe (s) What will be the coefficient in front of CO in the balanced chemical equation? If there is no coefficient in front of CO in the balanced equation, enter 1 as the answer.

[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.

How much (in gram) of HCl is required to produce 21.45 g of  AlCl3 if the percentage yield for the following reaction is 61.24% ? Enter your answer without units. Molar masses (in g/mol):Al = 26.98H2 = 2.016HCl = 36.46AlCl3 = 133.34 2Al(s) + 6 HCl (aq)  ⟶⟶  2 AlCl3(s) + 3H2(g)

For the reaction Ti(s) + 2 F2 (g) → TIF4(s) compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants.

Balance the following chemical equation (using the number "1" if the blank normally is left unfilled). Na (s) + NaF (s) F₂ (g) ---->

Do not give handwriting solution.

Hydrogen fuel can be generated using a process called coal gasification. Hydrogen gas is formed by the reaction of carbon, excess oxygen and excess water.                         3C (from coal) + O2 + H2O → H2 + 3CO If this process has an 84.22% yield, what mass of coal (65.5%C by mass) is needed to generate 1.33 kg of hydrogen?