The reaction of lithium aluminum hydride with acetone to produce isopropyl alcohol is shown below. LIAIH 4 Lithium Aluminum Hydride Molecular Weight: 37.95 4 Acetone Chemical Formula: C3H6O Molecular Weight: 58.08 H₂O 4 OH IsoPropyl Alcohol Chemical Formula: C3H₂O Molecular Weight: 60.10 Based on this reaction determine the theoretical yield of isopropyl alcohol given 55.42 grams of lithium aluminum hydride and an excess of acetone.

The theoretical yield of CCl4 is 50 g. If the actual yield from the reaction is 38 g of CCl4, what is the percent yield of CCl4? PY= (Actual/Theoretical)x 100

Combining 0.266 mol Fe,O, with excess carbon produced 20.0 g Fe. Fe, O, + 3 C → 2 Fe + 3 CO What is the actual yield of iron in moles? actual yield: mol What is the theoretical yield of iron in moles? theoretical yield: mol

Consider the following balanced equation, an important reaction in the industrial manufacture of phosphorus pentachloride:PCl3(g) + Cl2(g) → PCl5(g)This reaction has a known yield of PCl5 of 66.3%. You are a chemical engineer tasked with producingPCl5. Determine the actual mass of phosphorus pentachloride formed when you react 61.3 kg ofmolecular chlorine with an excess of phosphorus trichloride. (P: 30.97 g/mol; Cl: 35.45 g/mol)

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?

Methanol has tremendous potential to be used as an alternate fuel. Carbon monoxide gas reacted with hydrogen gas can be used to produce methanol.A student reacted 49.7 g of H2(g) with excess CO(g) to produce methanol.If his percent yield was 47.7%, calculate the mass (in g) of CH3OH(l) that he collected in the experiment.Hint: Write a balanced chemical reaction equation.Do not show your work in the space provided.Record only your final answer with the correct number of significant digits and the proper units.

Sulfur dioxide gas (SO2) reacts with excess oxygen gas (O2) and excess liquid water (H2O) to form liquid sulfuric acid (H2SO4). In the laboratory, a chemist carries out this reaction with 67.2 L of sulfur dioxide and gets 250 g of sulfuric acid. Write a balanced equation for the reaction. Calculate the theoretical yield of sulfuric acid. Calculate the percent yield of the reaction. (One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.)

The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: N₂(g) + O₂(g) → 2 NO(g) If 5.220 g N₂ is mixed with 9.660 g O₂, calculate the theoretical yield (g) of NO produced by the reaction. g

Complete combustion of 3.703.70 g of a hydrocarbon produced 12.012.0 g of CO2 and 3.703.70 g of H2O. What is the empirical formula for the hydrocarbon

According to the following reaction, how many grams of hydrofluoric acid will be formed upon the complete reaction of 26.4 grams of water with excess silicon tetrafluoride? silicon tetrafluoride (s) + water (I) --> hydrofluoric acid (aq) + silicon dioxide (s) O58.6g O 2.9g O 14.7g 20.2g