14. Iron metal is used extensively in the manufacture of automobiles. It can be produced by the reaction between iron (III) oxide (iron ore) and carbon monoxide: Fe:O3 (s) + 3 CO (g) 2 Fe (s) + 3 CO2 (g) Calculate the percent yield of this reaction if 1.56 kg of iron ore and 945 g of carbon monoxide actually produce 488 g of iron metal.

For the following reaction, 5.68 grams of chlorine gas are mixed with excess phosphorus (P4) . The reaction yields 5.34 grams of phosphorus trichloride .phosphorus (P4) ( s ) + chlorine ( g ) phosphorus trichloride ( l ) What is the theoretical yield of phosphorus trichloride ? grams What is the percent yield for this reaction ? %

Consider the balanced chemical equation: 3 H₂(g) + N₂(g) → 2 NH₃(g) If 46.8 g H₂ and 179.4 g N₂ are mixed to form NH₃, which of the following substances is the limiting reactant?   A) nitrogen (N₂) B) hydrogen (H₂) C) ammonia (NH₃)

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

Sodium and chlorine react to form sodium chloride:   What is the theoretical yield of sodium chloride for the reaction of 32.0 g Na with 107.2 g Cl2?     1.40 x 104 g NaCl     35.4 g NaCl     122 g NaCl     81.2 g NaCl

Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide at high temperatures, according to the following reaction.   NH3 (g) + CuO (s) → N2 (g) + Cu (s) + H2O (g)  What is the theoretical yield of solid copper that should form when 18.1 g of NH3 is reacted with 90.4 g of CuO?

For the following reaction, 3.02 grams of carbon monoxide are mixed with excess sulfur. The reaction yields 2.68 grams of sulfur dioxide. sulfur (s) + carbon monoxide (g) →sulfur dioxide (g) + carbon (s) What is the theoretical yield of sulfur dioxide ? grams What is the percent yield of sulfur dioxide ?

Determine the theoretical yield of HCl, if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction. (The molar mass of BCl3 = 117.16 g/mol)   BCl3(g) + 3 H2O(l)  →  H3BO3(s) + 3 HCl(g)

Al2Cl6 is made by treating scrap metal with chlorine gas according to the following equation: 2 Al (s)   +   3 Cl2 (g)   ⟶⟶   Al2Cl6 (s)  In the reaction of 45.9 g Al with 212.5 g Cl2, determine the limiting reactant and theoretical yield of the product. The limiting reactant is? The theoretical yield of Al2Cl6 is?.  Round the answer to 1 decimal place. If the reaction produces 139.4 g Al2Cl6, calculate the percent yield of the reaction. ? %.     Round the answer to 1 decimal place.