Consider the balanced chemical reaction below. What is the maximum amount of grams of Fe that can be produced from 33.4 g iron(III) oxide mixed with 47.2 g carbon monoxide?

Consider the following balanced chemical equation:    2Cu2O(s) + O2(g)  →  4CuO(s)   Determine the mass (in g) of CuO formed if 50.1 g of Cu2O reacts with 50.1 g of O2.  g CuO

4. When a solution containing 15.0 g of lead (II) nitrate and a solution containing 15.0 g of potassium iodide are mixed, a yellow precipitate of lead (II) iodide is formed. If 6.68 g of the precipitate are formed, what is the percent yield for the reaction?

An aqueous solution containing 9.55 g9.55 g of lead(II) nitrate is added to an aqueous solution containing 5.77 g5.77 g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. What is the limiting reactant? The percent yield for the reaction is 83.6%83.6%. How many grams of the precipitate are formed? How many grams of the excess reactant remain?

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

Consider the following balanced equation for the combustion of butane, a fuel often used in lighters.2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H2O(g)Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed.   Mass C4H10 Mass O2 Mass CO2 Mass H2O _____ 2.11 g _____ _____ 5.32 g _____ _____ _____ _____ _____ 13.12 g _____ _____ _____ _____ 8.44 g 252 mg _____ _____ _____ _____ _____ 198 mg _____

A chemist goes into the lab and performs an experiment in which a mixture of 8.47 grams of Zn and 6.03 g of sulfur are reacted.  Before starting the experiment they perform the following calculations to predict the maximum (theoretical) yield of zinc sulfide that could be produced.   They obtain an actual yield of 8.25 grams of zinc sulfide.   Calculate their percent yield to one decimal place.

If 36.0 g of C3H8 and 112 g of O2 are placed in a closed container and the mixture is ignited, what is the maximum mass of CO2 that could be produced? The other product of the reaction is water.     68.9 g     74.7 g     86.8 g     92.4 g     108 g

For the following reaction, 23.1 grams ofcarbon disulfide are allowed to react with89.2 grams of chlorine gas .carbon disulfide ( s ) + chlorine ( g ) carbon tetrachloride ( l ) + sulfur dichloride ( s )What is the maximum amount of carbon tetrachloride that can be formed? grams What is the FORMULA for the limiting reagent?   What amount of the excess reagent remains after the reaction is complete? grams

A 18.2 g of iron metal reacts with excess oxygen gas to produce 47.9 g of Fe3O4. The reaction between these two substances are written as:   ____ Fe(s) + ____ O2(g) → _____ Fe3O4 (s) Balance the chemical equation. Calculate the molar mass of O2 and Fe3O4. If the 43.72 g of Fe3O4 was produced, what is the percent yield of this reaction?