3. Chemical Reactions

The following reaction shows the mineral ilmenite, FeTiO₃, being reacted with chlorine gas and sand in order to extract titanium (IV) chloride. 

FeTiO₃ (s)  +  3 Cl₂ (g)  +  3 C (s) → 3 CO (g)  +  FeCl₂ (s)  +  TiCl₄ (g) 

Assuming a 100% yield, how many grams of titanium (IV) chloride can be extracted when reacting 18.0 g ilmenite, 30.0 g Cl₂ and 40.0 g C?

Lithium solid reacts with oxygen gas to create lithium oxide solid.

4 Li (s)  +  O₂ (g)  →  2 Li₂O (s)

If 131 g of Li are allowed to react with 215 g O₂, how many kilograms of the excess reactant would remain?

Nitrogen 1N22 and hydrogen 1H22 react to form ammonia 1NH32. Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. (d) Are any reactant molecules left over, based on the diagram?

Nitrogen 1N22 and hydrogen 1H22 react to form ammonia 1NH32. Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. (d) If so, how many of which type are left over?

How many N2 molecules are left over?

Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. (a) How many molecules of NO2 can be formed, assuming the reaction goes to completion?

A hydrogen-filled balloon is ignited and 1.50 g of hydrogen is reacted with 12.0 g of oxygen. How many grams of water vapor form? (Assume that water vapor is the only product.)

Calculate the theoretical yield of product (in moles) for each initial amount of reactants. 3 Mn(s) + 2 O2( g)¡Mn3O4(s) b. 4 mol Mn, 7 mol O2

Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq)¡FeCl2(s) + H2S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?

(c) Why should you base your choice of which compound is the limiting reactant on its number of initial moles, not on its initial mass in grams?

(b) Why are the amounts of products formed in a reaction determined only by the amount of the limiting reactant?

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. (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 NaOH1s2 + CO21g2¡Na2CO31s2 + H2O1l2 How many moles of the excess reactant remain after the completion of the reaction?

Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH1s2 + CO21g2¡Na2CO31s2 + H2O1l2 How many moles of Na2CO3 can be produced?

Limestone (CaCO₃) reacts with hydrochloric acid according to the equation CaCO₃ + 2 HCl ---> CaCl₂ + H₂O + CO₂. If 1.00 mol of CO₂ has a volume of 22.4 L under the reaction conditions, how many liters of gas can be formed by reaction of 2.35 g of CaCO₃ with 2.35 g of HCl? Which reactant is limiting?

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?

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 Which is the limiting reactant when 0.500 mol Al1OH23 and 0.500 mol H2SO4 are allowed to react?

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 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?

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 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?

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.

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 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?

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.

When a mixture of 10.0 g of acetylene 1C2H22 and 10.0 g of oxygen 1O22 is ignited, the resulting combustion reaction produces CO2 and H2O. (c) How many grams of CO2 are present after the reaction is complete?

When a mixture of 10.0 g of acetylene 1C2H22 and 10.0 g of oxygen 1O22 is ignited, the resulting combustion reaction produces CO2 and H2O. (c) How many grams of C2H2 are present after the reaction is complete?

When magnesium metal is burned in air (Figure 3.6), two products are produced. One is magnesium oxide, MgO. The other is the product of the reaction of Mg with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas. (d) Magnesium nitride can also be formed by reaction of the metal with ammonia at high temperature. Write a balanced equation for this reaction. If a 6.3-g Mg ribbon reacts with 2.57 g NH31g2 and the reaction goes to completion, which component is the limiting reactant? What mass of H21g2 is formed in the reaction?

Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N₂(g) + 3H₂(g) ⟶ 2NH₃(g) there are four molecules of nitrogen and nine molecules of hydrogen present in the diagram. When the reaction is complete, how many molecules of NH₃ are produced?

1 moles of mn reacts with 1 moles of O₂. What is the theoretical yield of the product? 𝗠𝗻(𝘀) + 𝗢₂(𝗴) → 𝗠𝗻𝗢₂(𝘀)

What is the maximum mass of S₈ that can be produced by combining 76.0 g of each reactant?

What is the maximum mass of s8 that can be produced by combining 83.0 g of each reactant?

A chemical reaction involving substances a and b stops when b is completely used. B is the

If a reactant is in excess, why do we not worry about the mole ratios involving that reactant?