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Chemical reactions: Limiting Reagent & Percent Yield

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Wize University Chemistry Textbook > Stoichiometry

Atoms, Molecules, and the Mole!

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Wize University Chemistry Textbook > Stoichiometry

Percent Yield

4 Activities

Wize University Chemistry Textbook > Stoichiometry

Limiting Reagents

5 Activities

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Iron oxidizes when exposed to oxygen to form iron oxide according to the following equation:
Fe (s) + O2 (g) ​→ Fe2​O3​ (s)

352g of pure iron is exposed to 12.0 mols of O2, and after a period of time, 46.7 g of iron oxide (rust) is collected.

a) What is the limiting reagent in this reaction?

b) What is the percent yield?

c) How many Fe atoms are present in the rust produced



More Atoms, Molecules, and the Mole! Questions:
Combustion, Stoichiometry
What mass of KClO3 is required to produce proper amount of O2 needed to achieve complete combustion of 78.88 g CH4?
2 KClO3 → 2 KCl + 3 O2
Given that the molar mass of X is 170.12 g mol-1, how many molecules of X are present in a tablet that contains 100 mg of X?
Calculate the molar mass of H2O
Molecules: Molar mass
Calculate the number of moles of each compound:
a. 18.5 g of MgCO3
b. 2.36 g of NF3
Stoichiometry: Chemical formula
How many carbon atoms are in 10.00 mL of ethanol ( CH3CH2OH)?
The density of ethanol is 0.789 g/mL.
Practice: Finding the Number of Moles of Iron
Calculate the number of moles of Iron atoms in 14.1 g of iron oxide, Fe2O3
Introduction to General Chemistry
Answer the following questions concerning benzoic acid (C7H6O2).
a) Calculate the number of moles in a 7.50 x 10-2 g sample of benzoic acid.
b) Calculate the number of molecules of benzoic acid in the 7.50 x 10-2 g sample.
Stoichiometry: Moles, atomic mass
Acetominophen (C8H9NO2) is a common drug used to treat pain and fever. It is the main component of common trade names such as Tylenol.
a) Calculate the molar mass of acetominophen.
b) How many moles of acetominophen are there in 250.0 g of this compound?
Converting Mass to Number of Atoms
Calculate the number of nitrogen atoms in 2.25 g of bismuth(III) nitrate. (Enter your answer in scientific notation in nitrogen atoms, for example 1.23⋅10181.23\cdot10^{18})
How many grams of oxygen are in 22 mL of water? Remember that the density of water is 1.0 g/mL
How many moles of ammonia (NH3) are in 2.4g of ammonia?
Chemical formula: Moles
Which of the following quantities is not equivalent to 5 mg of sodium bicarbonate,NaHCO3?
Stoichiometry: Finding the Number of Moles of Iron
Calculate the number of moles of iron atoms in 14.1 g of iron oxide, Fe2O3
Atoms: Avogadro's Number
How many C\text{C} atoms are there in 260 g of H2CO3\text{H}_2\text{CO}_3?
Stoichiometry: Molar mass and Avogadro's Number
How many hydrogen atoms are in exactly 2 g of hydrazinium sulfate, N2H6SO4?
More Percent Yield Questions:
Percent Yield
If the yield for the following reaction is 45%, how many moles of KClO3 are needed to produce 1 mol of O2?
2KClO3(s) → 2KCl(s) + 3O2(g)
Stoichiometry
Consider the following reaction:
2 Ca3(PO4)2 (s) + 10 C (s) + 6 SiO2 (s) → 6 CaSiO3 (s) + 10 CO (g) + P4 (l)
An initial reaction mixture contains 15.0 g Ca3(PO4)2, 10.0 g SiO2, and 4.00 g C. After the reaction, 2.17 g P4 is obtained. What is the percent yield for this experiment?
Chemical Reactions: Actual Yield
Consider the following reaction:
PCℓ3+Cℓ2→PCℓ5PC\ell_3 + C\ell_2 \to PC\ell_5
If the yield of the reaction is 76.5 %, what is the mass of PCl5 , in grams, obtained from the reaction of 27.0 g of PCl3 with excess Cl2? Give your answer to one decimal place; do not include units in your answer.
Stoichiometry: Percent yield
In the balanced reaction below, a student reacts 1.25g of copper with 5.0mL of 12.0mol/L HCl.
Cu(s)+2HCℓ(aq)→CuCℓ2(aq)+H2(g)Cu(s)+ 2HC \ell(aq)\to CuC\ell_2(aq) +H_2(g)
Stoichiometry: Limiting Reagents
Vanillin acetate is a synthetic flavoring agent used to mimic the natural flavor of vanilla in candies, beverages, ice creams, and baked goods. You only need 10-30 ppm concentrations of vanillin acetate to flavor most foods! The preparation of this compound is described by the balanced reaction scheme below. Use the data provided to answer the following questions.
Stoichiometry 2
An unknown hydrocarbon contains 40.0% C and 6.66% H by weight.
a. What is the empirical formula of the compound?
b. What is the molecular formula if molecular weight of the compound is 180 gmol-1?
Stoichiometry
Consider the following reaction:
2 Ca3(PO4)2 (s) + 10 C (s) + 6 SiO2 (s) → 6 CaSiO3 (s) + 10 CO (g) + P4 (l)
An initial reaction mixture contains 15.0 g Ca3(PO4)2, 10.0 g SiO2, and 4.00 g C. After the reaction, 2.17 g P4 is obtained. What is the percent yield for this experiment?
Consider the two following reactions:
CS2 + 3Cl2 → CCl4 (l)+ S2Cl2 (l) 60% yield
3 CCl4 (l) + 2 SbF3 (s) → 3 CCl2F2 (g) + 2SbCl3 (s) 80% yield
Consider the following reaction:
PCl3 + Cl2 = PCl5
If the yield of the reaction is 76.5 %, what is the amount of PCl5 obtained from 27.0 g of PCl3?
Precipitation
Zinc reacts with silver nitrate according to the following equation:
Zn (s) + 2AgNO3 (aq) → Zn(NO3)2 (aq) + 2Ag (s)
The concentration of AgNO3 solution is 1.330 molsL-1. 100 g Zn was added to 1.000 L of this solution and 90.0 g Ag is collected. What is the percent yield of this reaction?
Precipitation
CaSO4 can be converted to CaO at high temperature by the following two step procedure:
CaSO4 (s) + 4C → CaS (l) + 4CO (g)
CaS (l) + 3CaSO4 (s) → 4CaO (s) + 4SO2
Percent Yield
Sodium carbonate is an inexpensive compound that has a variety of applications. It is used in glass and paper manufacturing as well as in common foods like ramen noodles. The production of sodium carbonate occurs in a two step reaction as shown below:
1. H2O + NaCl + NH3 + CO2 → NH4Cl + NaHCO3
2. 2NaHCO3 → Na2CO3 + CO2 + H2O
Percent Yield
If the yield for the following reaction is 45%, how many moles of KClO3 are needed to produce 1 mol of O2?
2KClO3(s) → 2KCl(s) + 3O2(g)
CHEM 1011 (Dalhousie) - Stoichiometry
2. In the unbalanced reaction below, a student reacts 1.25 g of copper with 5.0 mL of 12.0 M HCl.
Cu (s)    +    HCl (aq)    →    CuCl2 (aq)    +    H2 (g)Cu\ \left(s\right)\ \ \ \ +\ \ \ \ HCl\ \left(aq\right)\ \ \ \ \rightarrow\ \ \ \ CuCl_2\ \left(aq\right)\ \ \ \ +\ \ \ \ H_2\ \left(g\right)
a) Calculate the theoretical yield of hydrogen gas produced in grams.
Stoichiometry: Limiting reagents
3. Consider the chemical reaction described below:
Ca3(PO4)2 (s)    +    C (s)    +    SiO2 (s)    →    CaSiO3 (s)    +    CO (g)    +    P (l)Ca_3\left(PO_4\right)_2\ \left(s\right)\ \ \ \ +\ \ \ \ C\ \left(s\right)\ \ \ \ +\ \ \ \ SiO_2\ \left(s\right)\ \ \ \ \rightarrow\ \ \ \ CaSiO_3\ \left(s\right)\ \ \ \ +\ \ \ \ CO\ \left(g\right)\ \ \ \ +\ \ \ \ P\ \left(l\right)
a) What is the limiting reagent for this reaction if an initial reaction mixture contains 1325 kg of calcium phosphate, 300 kg of carbon and 890 kg of silicon dioxide.
Chemical Reactions: Limiting Reagent
Based on the unbalanced chemical reaction below:
NaNO2 (s)    +    O2 (g)    →    NaNO3 (s)NaNO_2\ \left(s\right)\ \ \ \ +\ \ \ \ O_2\ \left(g\right)\ \ \ \ \rightarrow\ \ \ \ NaNO_3\ \left(s\right)
a) Calculate the mass of sodium nitrate if 10.25 g of sodium nitrite is reacted with 7.55 g of oxygen gas.
Chemical Reactions: Limiting Reagent & Percent Yield Practice
Iron oxidizes when exposed to oxygen to form iron oxide according to the following equation:
Fe + O2 ​→Fe2​O3​
352g of pure iron is exposed to 12.0 mols of O2, and after a period of time 46.7 g of iron oxide (rust) is collected.
Chemical Reactions: Percent Yield
If the yield for the following reaction is 45%, how many moles of KClO3 are needed to produce 1 mol of O2?
2KClO3(s) -> 2KCl(s) + 3O2(g)
Stoichiometry: Mass Percentage
How many grams of PCl3 are needed to produce 10g of POCl3 using an excess of hydrogen peroxide assuming a typical reaction yield of 78%?
PCl3+H2O2→POCl3+H2OPCl_3+H_2O_2\rightarrow POCl_3+H_2O
Stoichiometry: Percent yield
Consider the following unbalanced reaction:
C4H8O2+O2→CO2+H2O\rm C_4H_8O_2 +O_2 \to CO_2 + H_2O
If 36.00 g of C4H8O2\rm C_4H_8O_2 is burned, what mass of water would be collected if the reaction yield was 76%?
Stoichiometry: Percent Yield
A compound with the formula C7H8O3\text{C}_7\text{H}_8\text{O}_3 is burned to completion in excess O2\text{O}_2. If 18.0g of the organic compound was consumed in the reaction, how many grams of H2O\text{H}_2\text{O} will be collected if the yield was 85%?
The potassium salt of benzoic acid, potassium benzoate (KC7H5O2, MM=160 g/mol) can be made by the action of potassium permanganate on toluene (C7H8, MM=92 g/mol). If the yield of potassium benzoate cannot realistically be expected to be more than 71%, what is the minimum number of grams of toluene needed to produce 11.5 g of potassium benzoate?
C7H8+2KMnO4→KC7H5O2+2MnO2+KOH+H2OC_7 H_8+2KMnO_4→KC_7 H_5 O_2+2MnO_2+KOH+H_2 O
Stoichiometry: Percent Yield
How many grams of PCl3 are needed to produce 10g of OPCl3 using an excess of hydrogen peroxide assuming a typical reaction yield of 78%?
PCl3​ + H2​O2 ​→ OPCl3​ + H2​O
Chemical Reactions: Limiting Reagent & Percent Yield Practice
Iron oxidizes when exposed to oxygen to form iron oxide according to the following equation:
Fe + O2 ​→Fe2​O3​
352g of pure iron is exposed to 12.0 mols of O2, and after a period of time 46.7 g of iron oxide (rust) is collected.
Percent Yield
If the yield for the following reaction is 45%, how many moles of KClO3 are needed to produce 1 mol of O2?
2KClO3(s) -> 2KCl(s) + 3O2(g)
Aspirin is produced by the reaction of salicylic acid, C7H6O3\rm C_7H_6O_3, and acetic anhydride, C4H6O3\rm C_4H_6O_3
C7H6O3(s)+C4H6O3(l)→C9H8O4(s)+C2H4O2(l)\rm C_7H_6O_3(s)+C_4H_6O_3(l)\rightarrow C_9H_8O_4(s)+C_2H_4O_2(l)
If 2.04 g of C9H8O4\rm C_9H_8O_4 is produced from the reaction of 3.03 g C7H6O3\rm C_7H_6O_3 and 4.01 g C4H6O3\rm C_4H_6O_3, what is the percent yield?
More Limiting Reagents Questions:
Stoichiometry and Limiting Reagent
Consider the following balanced equation:
2 NH3 (g) + 3 CuO (s) → N2 (g) + 3 Cu (s) + 3 H2O (l)
A reaction mixture contains 18.1 g NH3 and 90.4 g CuO. How much of the limiting reagent in (g's) is remaining?
Chemical reactions: Limiting Reagent
Sodium metal reacts with water to give sodium hydroxide and hydrogen gas as per the following unbalanced equation:
Na(s)+H2O(l)→NaOH(aq)+H2(g)Na(s)+H_2O(l)\rightarrow NaOH(aq)+H_2(g)
If 1.00 g of sodium were reacted with 0.786 g of water which species would be the limiting reagent?
Stoichiometry and Limiting Reagent
Consider the following balanced equation:
2 NH3 (g) + 3 CuO (s) → N2 (g) + 3 Cu (s) + 3 H2O (l)
A reaction mixture contains 18.1 g NH3 and 90.4 g CuO. How much of the limiting reagent in (g's) is remaining?
Stoichiometry: Limiting Reagents
Vanillin acetate is a synthetic flavoring agent used to mimic the natural flavor of vanilla in candies, beverages, ice creams, and baked goods. You only need 10-30 ppm concentrations of vanillin acetate to flavor most foods! The preparation of this compound is described by the balanced reaction scheme below. Use the data provided to answer the following questions.
Sodium metal reacts with water to give sodium hydroxide and hydrogen gas as per the following unbalanced equation:
Na(s)+H2O(l)→NaOH(aq)+H2(g)Na(s)+H_2O(l)\rightarrow NaOH(aq)+H_2(g)
If 1.00 g of sodium were reacted with 0.786 g of water which species would be the limiting reagent?
Gas Stoichiometry and Limiting Reagent
Consider the following equation:
4NH3(g) + 7O2(g) → 4NO2(g) + 6H2O(l)
3 L NH3 and 7 L O2 were reacted at 350 °C and 111 kPa. How much NO2 can be produced?
Stoichiometry: Yield
What is the maximum amount of iodine gas (in moles) that can be formed if 1.00 mole of manganese (IV) oxide was allowed to react with 2.00 moles of hydroiodic acid to from manganese(II) iodide, iodine gas, and water?
Chemical reactions: Limiting Reagent & Percent Yield
Iron oxidizes when exposed to oxygen to form iron oxide according to the following equation:
Fe (s) + O2 (g) ​→ Fe2​O3​ (s)
352g of pure iron is exposed to 12.0 mols of O2, and after a period of time, 46.7 g of iron oxide (rust) is collected.
Stoichiometry: Limiting reagents
3. Consider the chemical reaction described below:
Ca3(PO4)2 (s)    +    C (s)    +    SiO2 (s)    →    CaSiO3 (s)    +    CO (g)    +    P (l)Ca_3\left(PO_4\right)_2\ \left(s\right)\ \ \ \ +\ \ \ \ C\ \left(s\right)\ \ \ \ +\ \ \ \ SiO_2\ \left(s\right)\ \ \ \ \rightarrow\ \ \ \ CaSiO_3\ \left(s\right)\ \ \ \ +\ \ \ \ CO\ \left(g\right)\ \ \ \ +\ \ \ \ P\ \left(l\right)
a) What is the limiting reagent for this reaction if an initial reaction mixture contains 1325 kg of calcium phosphate, 300 kg of carbon and 890 kg of silicon dioxide.
Chemical Reactions: Limiting Reagent & Percent Yield Practice
Iron oxidizes when exposed to oxygen to form iron oxide according to the following equation:
Fe + O2 ​→Fe2​O3​
352g of pure iron is exposed to 12.0 mols of O2, and after a period of time 46.7 g of iron oxide (rust) is collected.
Stoichiometry: Limiting reagents
Ammonia, NH3, and borane, BH3, react to form a Lewis adduct, ammonia borane as shown below.
NH3(sol)+BH3(sol)→NH3BH3(s)NH_{3(sol)} + BH_{3(sol)} \rightarrow NH_3BH_{3(s)}
If 24 mL of a 0.74 M solution of ammonia is mixed with 12 mL of a 1.8 M solution of borane what is the maximum mass of ammonia borane that can be produced?
Stoichiometry: Limiting Reagents
When we are solving a stoichiometry problem and are given a balanced reaction, the limiting reagent is the reagent that...
(There are 2 correct answers)
Stoichiometry: Limiting reagents
17g of P4 reacts with 64g of oxygen, O2 as described below in the UNBALANCED reaction. What is the maximum amount of P4O6 that can be formed?
P4(s)+O2(g)→P4O6(s)P_{4(s)}+O_{2(g)}\rightarrow P_4O_{6(s)}
Chemical Reaction: Limiting Reagent
If 12 g of sodium is mixed with 0.64 g of H2 and 17 g of O2 which reagent will be limiting in the reaction shown below?
2 Na(s)+O2(g)+H2(g)→2 NaOH2\ Na_{(s)}+O_{2(g)}+H_{2(g)}\rightarrow 2\ NaOH
Chemical Reactions: Limiting Reagents
Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor:
4NH3+5O2→4NO+6H2O\rm 4NH_3+5O_2\rightarrow4NO+6H_2O
When 20.0 g NH3\rm NH_3 and 50.0 g O2\rm O_2 are allowed to react, which is the limiting reagent?
Chemical Reactions: Limiting Reagents
Magnesium metal reacts with HCl\text{HCl} to produce magnesium chloride (MgCl2\text{MgCl}_ 2 ) and hydrogen gas (H2\text{H}_2 ). If 0.568 g of magnesium are reacted with 75.0 mL of a 0.450 M solution of HCl\text{HCl}, how much magnesium metal will remain after the reaction is complete?
Chemical Reactions: Limiting Reagent & Percent Yield Practice
Iron oxidizes when exposed to oxygen to form iron oxide according to the following equation:
Fe + O2 ​→Fe2​O3​
352g of pure iron is exposed to 12.0 mols of O2, and after a period of time 46.7 g of iron oxide (rust) is collected.
Chemical Reactions: Limiting Reagents
Consider the following unbalanced reaction
Which reagent is in excess?
Chemical reactions: Limiting Reagent
Sodium metal reacts with water to give sodium hydroxide and hydrogen gas as per the following unbalanced equation:
Na(s)+H2O(l)→NaOH(aq)+H2(g)Na(s)+H_2O(l)\rightarrow NaOH(aq)+H_2(g)
If 1.00 g of sodium were reacted with 0.786 g of water which species would be the limiting reagent?