(b) Why is the actual yield in a reaction almost always less than the theoretical yield?

(c) Can a reaction ever have 110% actual yield?

Consider the mixture of ethanol, C2H5OH, and O2 shown in the accompanying diagram. (b) Which reactant is the limiting reactant?

Consider the mixture of ethanol, C2H5OH, and O2 shown in the accompanying diagram. (c) How many molecules of CO2, H2O, C2H5OH, and O2 will be present if the reaction goes to completion?

Consider the mixture of propane, C3H8, and O2 shown here. (a) Write a balanced equation for the combustion reaction that occurs between propane and oxygen.

Consider the mixture of propane, C3H8, and O2 shown here. (c) How many molecules of CO2, H2O, C3H8, and O2 will be present if the reaction goes to completion?

Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO₂(g) → Na₂CO₃(s) + H₂O(l) Which is the limiting reactant when 1.85 mol NaOH and 1.00 mol CO₂ are allowed to react?

Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO₂(g) → Na₂CO₃(s) + H₂O(l) How many moles of Na₂CO₃ can be produced?

Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH1s2 + CO21g2¡Na2CO31s2 + H2O1l2 How many moles of the excess reactant remain after the completion of the reaction?

Aluminum hydroxide reacts with sulfuric acid as follows: 2 Al1OH231s2 + 3 H2SO41aq2¡Al21SO4231aq2 + 6 H2O1l2 Which is the limiting reactant when 0.500 mol Al1OH23 and 0.500 mol H2SO4 are allowed to react?

Aluminum hydroxide reacts with sulfuric acid as follows: 2 Al1OH231s2 + 3 H2SO41aq2¡Al21SO4231aq2 + 6 H2O1l2 How many moles of Al21SO423 can form under these conditions?

Aluminum hydroxide reacts with sulfuric acid as follows: 2 Al1OH231s2 + 3 H2SO41aq2¡Al21SO4231aq2 + 6 H2O1l2 How many moles of the excess reactant remain after the completion of the reaction?

The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between sodium bicarbonate 1NaHCO32 and citric acid 1H3C6H5O72: 3 NaHCO31aq2 + H3C6H5O71aq2¡ 3 CO21g2 + 3H2O1l2 + Na3C6H5O71aq2 In a certain experiment 1.00 g of sodium bicarbonate and 1.00 g of citric acid are allowed to react. (a) Which is the limiting reactant? (b) How many grams of carbon dioxide form? (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed?

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2 In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (a) Which is the limiting reactant?

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2 In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed?

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH₃ to NO: 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g) In a certain experiment, 2.00 g of NH₃ reacts with 2.50 g of O₂. (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.50 g of sodium carbonate is mixed with one containing 5.00 g of silver nitrate. How many grams of sodium carbonate are present after the reaction is complete? How many grams of sodium nitrate are present after the reaction is complete?

Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.50 g of sodium carbonate is mixed with one containing 5.00 g of silver nitrate. How many grams of silver carbonate are present after the reaction is complete?

Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. If 5.00 g of sulfuric acid and 5.00 g of lead(II) acetate are mixed, calculate the number of grams of sulfuric acid and grams of acetic acid present in the mixture after the reaction is complete.

Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. If 5.00 g of sulfuric acid and 5.00 g of lead(II) acetate are mixed, calculate the number of grams of lead(II) acetate present in the mixture after the reaction is complete.

When benzene 1C6H62 reacts with bromine 1Br22, bromobenzene 1C6H5Br2 is obtained: C6H6 + Br2¡C6H5Br + HBr (a) When 30.0 g of benzene reacts with 65.0 g of bromine, what is the theoretical yield of bromobenzene?

When benzene 1C6H62 reacts with bromine 1Br22, bromobenzene 1C6H5Br2 is obtained: C6H6 + Br2¡C6H5Br + HBr (b) If the actual yield of bromobenzene is 42.3 g, what is the percentage yield?

When ethane 1C2H62 reacts with chlorine 1Cl22, the main product is C2H5Cl, but other products containing Cl, such as C2H4Cl2, are also obtained in small quantities. The formation of these other products reduces the yield of C2H5Cl. (a) Calculate the theoretical yield of C2H5Cl when 125 g of C2H6 reacts with 255 g of Cl2, assuming that C2H6 and Cl2 react only to form C2H2Cl and HCl. (b) Calculate the percent yield of C2H5Cl if the reaction produces 206 g of C2H5Cl.

Hydrogen sulfide is an impurity in natural gas that must be removed. One common removal method is called the Claus process, which relies on the reaction: 8 H2S1g2 + 4 O21g2¡S81l2 + 8 H2O1g2 Under optimal conditions the Claus process gives 98% yield of S8 from H2S. If you started with 30.0 g of H2S and 50.0 g of O2, how many grams of S8 would be produced, assuming 98% yield?

When hydrogen sulfide gas is bubbled into a solution of sodium hydroxide, the reaction forms sodium sulfide and water. How many grams of sodium sulfide are formed if 1.25 g of hydrogen sulfide is bubbled into a solution containing 2.00 g of sodium hydroxide, assuming that the sodium sulfide is made in 92.0% yield?

Write balanced chemical equations for (a) the complete combustion of acetone (CH₃COCH₃), a common organic solvent (b) the decomposition of solid mercury (I) carbonate into carbon dioxide gas, mercury, and solid mercury oxide

Write balanced chemical equations for (c) the combination reaction between nickel metal and chlorine gas.

If 2.0 mol CH3CH2CH2COOH, 2.0 mol C4H10, and 2.0 mol C6H6 are completely combusted in oxygen, which one produces the largest number of moles of H2O?

If 2.0 mol CH3CH2CH2COOH, 2.0 mol C4H10, and 2.0 mol C6H6 are completely combusted in oxygen, which one produces the least? Explain.