3. Chemical Reactions

Percent Yield

GCSE Chemistry - Percentage Yield  #33

The reduction of iron (III) oxide creates the following reaction:&nbsp;Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H2O (g)&nbsp;If the above reaction only went to 75% completion, how many moles of Fe2O3 were require to produce 0.850 moles of Fe?&nbsp;

The combustion of liquid ethanol (C2H5OH) produces carbon
dioxide and water. After 4.62 mL of ethanol (density =
0.789 g>mL) is allowed to burn in the presence of 15.55 g of oxygen
gas, 3.72 mL of water (density = 1.00 g>mL) is collected.
Determine the percent yield for the reaction. (Hint: Write a balanced equation
for the combustion of ethanol.)

Ammonia, NH3, reacts with hypochlorite ion, OCl–, to produce hydrazine, N2H4. How many grams of hydrazine are produced from 115.0 g NH3 if the reaction has a 81.5% yield? &nbsp;2 NH3 + OCl– → N2H­4 + Cl– + H2O

Acetic acid (CH3CO2H) reacts with isopentyl alcohol (C5H12O) to yield isopentyl acetate (C7H14O2), a fragrant substance with the odor of bananas. If the yield from the reaction of acetic acid with isopentyl alcohol is 45%, how many grams of isopentyl acetate are formed from 3.58 g of acetic acid and 4.75 g of isopentyl alcohol? The reaction is CH3CO2H + C5H12O ---> C7H14O2 + H2O

If 42.85 grams of salicylic acid reacts with excess acetic anhydride and produces 48.47 grams of aspirin, what is the percent yield of the reaction? (LO 3.6) 
(a) 88.40% 
(b) 64.69%
(c) 86.72% 
(d) 78.74%

What is the percent yield for a reaction in which 22.1 g Cu is isolated by reacting 45.5 g Zn with 70.1 g CuSO4? &nbsp;Zn (s)&nbsp;+&nbsp;CuSO4 (aq) → Cu (s) + ZnSO4 (aq)

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.

Silver sulfide, the tarnish on silverware, comes from the reaction of silver metal with hydrogen sulfide (H2S).The unbalanced equation is: 
Ag + H2S + O2 --> Ag2S + H2O Unbalanced 
If the reaction was used intentionally to prepare Ag2S, how many grams would be formed from 496 g of Ag, 80.0 g of H2S, and excess O2 if the reaction takes place in 90% yield? (LO 3.9) 
(a) 525 g 
(b) 1139 g
(c) 583 g 
(d) 1025

Cisplatin [Pt(NH3)2Cl2], a compound used in cancer treat-ment, is prepared by reaction of ammonia with potassium tetrachloroplatinate: K2PtCl4 + 2 NH3 ----> 2 KCl + Pt(NH3)2Cl2
How many grams of cisplatin are formed from 55.8 g of K2PtCl4 and 35.6 g of NH3 if the reaction takes place in 95% yield based on the limiting reactant?

Nickel(II) sulfate, used for nickel plating, is prepared by treat-ment of nickel(II) carbonate with sulfuric acid:
NiCO3 + H2SO4 --> NiSO4 + CO2 + H2O
(b) How many grams of NiSO4 are obtained if the yield is 78.9%?

Limiting Reactants and Percent Yield

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?

Percent Yield Example 1

Percent Yield Made Easy: Stoichiometry Tutorial Part 4

If 1.87 g of acetic acid (CH3COOH) reacts with 2.31 g of isopentyl alcohol (C5H12O) to give 2.96 g of isopentyl acetate (C7H14O2), what is the percent yield of the reaction?

Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen:
N2H4 + O2 --> N2 + 2 H2O
(b) How many grams of N2 are obtained if the yield is 85.5%?

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?

Urea (CH4N2O) is a common fertilizer that is synthesized by the
reaction of ammonia (NH3) with carbon dioxide:
2 NH3(aq) + CO2(aq)¡CH4N2O(aq) + H2O(l )
In an industrial synthesis of urea, a chemist combines 136.4 kg
of ammonia with 211.4 kg of carbon dioxide and obtains
168.4 kg of urea. Determine the limiting reactant. Determine the theoretical yield of urea. Determine the percent yield for the reaction.

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

Titanium occurs in the magnetic mineral ilmenite (FeTiO3),
which is often found mixed with sand. The ilmenite can be
separated from the sand with magnets. The titanium can then
be extracted from the ilmenite by the following set of reactions:
FeTiO3(s) + 3 Cl2( g) + 3 C(s)¡3 CO(g) + FeCl2(s) + TiCl4( g)
TiCl4( g) + 2 Mg(s)¡2 MgCl2(l ) + Ti(s)
Suppose that an ilmenite–sand mixture contains 22.8% ilmenite
by mass and that the first reaction is carried out with a 90.8%
yield. If the second reaction is carried out with an 85.9% yield,
what mass of titanium can be obtained from 1.00 kg of the
ilmenite–
sand mixture?

If 3.42 g of K2PtCl4 and 1.61 g of NH3 give 2.08 g of cispla-tin (Problem 3.81), what is the percent yield of the reaction?

How to Calculate Percent Yield and Theoretical Yield The Best Way - TUTOR HOTLINE

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?

Theoretical, Actual and Percent Yield Problems - Chemistry Tutorial

How To Calculate Theoretical Yield and Percent Yield

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. (c) If the actual yield of the reaction was 75% instead of 100%, how many molecules of each kind would be present after the reaction was over? <img src="https://lightcat-files.s3.amazonaws.com/problem_images/5d20a95e17df7951-1660650523781.jpg" alt="" />

Magnesium oxide can be made by heating magnesium metal in
the presence of oxygen. The balanced equation for the
reaction is:
2 Mg(s) + O2( g)¡2 MgO(s)
When 10.1 g of Mg reacts with 10.5 g O2, 11.9 g MgO is collected.
Determine the limiting reactant. Determine the theoretical yield. Determine the percent yield for the reaction.

Many computer chips are manufactured from silicon, which occurs
in nature as SiO2. When SiO2 is heated to melting, it reacts
with solid carbon to form liquid silicon and carbon monoxide
gas. In an industrial preparation of silicon, 155.8 kg of SiO2 reacts
with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine
the percent yield for the reaction.

Viridicatumtoxin B, C30H31NO10, is a natural antibiotic compound. 
It requires a synthesis of 12 steps in the laboratory. 
Assuming all steps have equivalent yields of 85%, which is 
the final percent yield of the total synthesis?

Aspirin can be made in the laboratory by reacting acetic anhydride
(C4H6O3) with salicylic acid (C7H6O3) to form aspirin
(C9H8O4) and acetic acid (C2H4O2). The balanced equation is:
C4H6O3 + C7H6O3¡C9H8O4 + C2H4O2
In a laboratory synthesis, a student begins with 3.00 mL of acetic
anhydride (density = 1.08 g/mL) and 1.25 g of salicylic acid.
Once the reaction is complete, the student collects 1.22 g of aspirin.
Determine the limiting reactant. Determine the theoretical yield of aspirin. Determine the percent yield for the reaction.

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

(a) Define the terms theoretical yield, actual yield, and percent
yield.

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[BOOK CHEM] Clutch Version

Empirical Formula

The empirical formula gives the relative number of atoms.&nbsp;

The Percent Yield determines how successful the product yield is in a chemical reaction.&nbsp;

Molecular Formula

The&nbsp;molecular formula gives the actual number of atoms.

Naming Ionic Compounds

An ionic compound is composed of a positive ion and a negative ion.&nbsp;

Functional Groups in Chemistry

The Functional Group is the portion of a molecule that is responsible for its chemical reactivity.&nbsp;

Naming Molecular Compounds

Molecular Compounds, also known as covalent compounds, contain only non-metals bonded together.&nbsp;

Naming Ionic Hydrates

An Ionic Hydrate is an ionic compound that is linked to at least one molecule of H2O.&nbsp;

Stoichiometry

Stoichiometry deals with the numerical relationship between compounds in a balanced chemical equation.

Writing Ionic Compounds

Determining the charges of a cation and anion are fundamental in Writing Ionic Compounds.

Polyatomic Ions

Polyatomic Ions are groups of multiple elements that possess a charge.

Balancing Chemical Equations

Balancing Chemical Equations is the first step in future chemical calculations.

Limiting Reagent

The Limiting Reagent represents the compound that is totally consumed in the reaction.&nbsp;

Combustion Analysis

Under Combustion Analysis, the empirical formula of a compound is determined through a combustion reaction.&nbsp;

Mass Percent

Mass Percent is the percentage of a particular element within a compound.&nbsp;

Combustion Apparatus

A Combustion Apparatus vaporizes a sample into gases to later determine its formula.

Naming Acids

Acids, for the most part, are covalent compounds that begin with a hydrogen.&nbsp;