Percent Composition from a Chemical FormulaThe percent composition of a compound can also be determined from the formula of thecompound. The subscripts in the formula are first used to calculate the mass of each element inone mole of the compound. That is divided by the molar mass of the compound and multipliedby 100%100%.mass of element in 1 mol% by mass =x 100%molar mass of compoundStep by StepCalculation of PercentComposition of a compoundExample:A certain newly synthesized compound is known to contain the elements zinc and oxygen. Whena 20.00g20.00g sample of the compound is decomposed, 16.07gof zinc remains. Determine thepercent composition of the compound.Step 1: List the known quantities and plan the problem.KnownMass of compound =20.00gMass of Zn=16.07gZnUnknownPercent Zn=?%Percent O=?%Step 2: Subtract to find the mass of oxygen in the compound. Divide each element's mass by themass of the compound to find the percent by mass.Mass of oxygen = 20.00 g – 16.07 g = 3.93 g O16.07 g Zn20.00 g% Zn =x 100% = 80.35% Zn3.93 g O20.00 g%0 =x 100% = 19.65% OStep 3: Conclude the result: The calculations make sense because the sum of the twopercentages adds up to 100%100%. By mass, the compound is mostly zinc.step 4Dichlorine heptoxide (Cl207)(Cl207) is a highly reactive compound used in some organicsynthesis reactions. Calculate the percent composition of dichlorine heptoxide. Follow thestep by step procedure shown above.

Given that - Dichlorine heptoxide , Cl2O7 , which is a highly reactive compound. The molar…

step 4 Dichlorine heptoxide (C1207)(C1207) is a highly reactive compound used in some organic synthesis reactions. Calculate the percent composition of dichlorine heptoxide. Follow the step by step procedure shown abo ve.

step 4 Dichlorine heptoxide (C1207)(C1207) is a highly reactive compound used in some organic synthesis reactions. Calculate the percent composition of dichlorine heptoxide. Follow the step by step procedure shown abo ve.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A sample of limestone and other soil materials was heated, and the limestone decomposed to give…

A: Given -> CaCO3(s) -----> CaO(s) + CO2(g) Weight of sample = 2.237 gm Weight of CO2 formed =…

Q: A 2.68 gram sample of a KCl and KCIO3 mixture was found to contain 0.01541 mol of KCIO3. What is the…

Q: If you have 42.5 moles of glucose (C6H₁206) approximately how many grams do you have? #3

Q: Another student performed the same percent composition of a hydrate experiment, but kens the…

A: 3a. The experiment was the determination of percent composition of hydrate.

Q: A particular compound is comprised only of the elements C, H, N, and Cl. Combustion analysis of…

A: Given that: Total mass of sample = 14.30 g Mass of CO2 = 31.22 g Mass of H2O = 6.764 g Mass % of N=…

Q: 5) 0.7971 g of molecule, X, is found to contain 3.0 x 1022 atoms. Deduce the identity of X. Given N…

A: Given: Mass of X2 = 0.7971 g Atoms of X2 = 3.0×1022 NA = 6.023×1023 mol-1

Q: C6H6 contaminates a water sample. The sample contains 0.000037% of the compound by mass. How much…

A: Mass percent = (Mass of solute/Mass of solution) x 100 Let us consider the mass percent of solution…

Q: A crucible is placed on a balance and is found to have a mass of 26.639 grams a sample of…

A: Mass of crucible = 26.639 g Mass of crucible + mass of Na2SO4·xH2O = 27.085 g Therefore mass of…

Q: A sample of Water, H2O, has a mass of 55 grams. Determine the number of moles in the sample.

Q: Using dimensional analysis, convert from 3.56 moles of CH3OH to the number of moles of O2 required

A: moles of CH3OH = 3.56 moles moles of O2 required = ?

Q: 8. Convert 37.482 g of N₂O4 to nitrogen atoms.

A: In one mole of any substance there are 6.023 * 1023 number of entities present.

Q: CALCULATIONS Answer the following in Question 1-2 involves the same process three different times.…

A: The objective of the first question is to convert the mass of NaHCO3 into moles. The molar mass of…

Q: Find the molar mass of CO(NH2)2-

A: Molar mass of compound is sum of atomic masses of constituent atoms . Atomic mass of C = 12.01…

Q: A water solution of sulfuric acid (H2SO4) has a density of 1.864 g/mL and is 73.0% H2SO4 by mass.…

Q: A crucible is placed on a balance and is found to have a mass of 26.639 grams a sample of…

A: Since on heating the compound, the mass of water will be lost as it will get vaporised Hence the…

Q: A chemist weighs 50.0 grams of solid NaOH. a) How many moles of NaOH are in the sample? [ Select ]…

Q: For the following reactions, determine the value of x (in mol). a. 4 C+ S8 → 4 CS2 mol 1.9 mol Sg…

Q: 8.15g of phosphorus reacts with bromine to form 71.22g of phosphorus tribromide. Calculate the…

Q: Given : 1CH4 (g) + 2O2 (g) —> 1 CO2 (g) + 2 H2O (g) Q. calculate the mass of c02 gas formed when…

Q: Nitric acid is used in the production of fertilizer as well as nitroglycerin. Convert 2.9 x 1021…

A: Since, we know that ; 1 mol of nitric acid contains 6.022 × 1023 molecules. So, 2.9 × 1021…

Q: Starting with 0.525 mol Li and 0.210 mol SOCI₂, determine the number of moles of each reactant and…

A: Recall the given reaction, 4 Li + 2 SOCl2 → 4 LiCl + S + SO2Initially…

Q: When burning butanol (C4H100), what mass (in g) of butanol must be reacted to produce 55.4 g of…

A: Mass (in g) of butanol must be reacted to produce 55.4 g of productsThe balanced equation for…

Q: When the following molecular equation is balanced using the smallest possible integer coefficients,…

A: The balanced molecular eqn is given by - 4NH3(g) + 5O2(g)---> 4NO (g) + 6H2O (g) When the…

Q: calculate the masses of both reactants and products assuming a 100% reaction. Na3PO3 +…

A: Stoichiometry, in balanced chemical reaction is defined by the ratio at which reactants are reacting…

Q: 1. What is the molecular formula for the unknown hydrate? 2. What is the percent mass of water in…

A: The molecular formula for the unknown hydrate is to be determined from the given experimental data.…

Q: . How many moles of Al(C 2 H 3 O 2 ) 3 contain 19mol O ? 6. Determine the % composition by mass of…

Q: A 14.590 g14.590 g sample of CaCl2CaCl2 was added to 12.028 g12.028 g of K2CO3K2CO3 and mixed in…

A: Determine limiting reagent:From the balanced chemical equation, 1 mol of CaCl2 and 1 mol of K2CO3…

Q: 1-Calculate the mass of compound required to prepare 100.00 mL of a 1.40x102 M CuCl2 ?.

A: Molecular weight of CuCl2 = 134.45 g mol-1 Formula Used 1. No of moles = volume × concentration 2.…

Q: If 5.3 g of hydrogen gas is reacted with 12.6 g of oxygen gas to produce water, the hydrogen is the…

A: Chemical reaction: 2 H2 + O2 ---> 2 H2O Mass of H2 = 5.3 g Mass of O2 = 12.6 g Molar mass of H2…

Q: FORMULAS FROM PERCENT COMPOSITION: 8. %Zn = 11.44%; %U = 41.64; %C = 16.81%; %H = 2.12%; %O = 27.9

Q: The maximum amount of Al2O3 that can be produced from 2.5 g of Al and 2.5 g of O2 is

A: Given, mass of Al (s) = 5.0 g mass of O2 (g) = 5.0 gNow, moles of Al (s) and O2 (g)…

Q: In a terrible accident, a solution consisting of 2.37 kg of nitric acid, HNO3, was spilled on the…

A: Given: The mass of HNO3 that was spilled = 2.37 kg The mass of Na2CO3 added = 2.00 kg We have to…

Q: Consider the following chemical reaction HCl (aq) + HgNO3 (aq) à Hg2Cl2 (s) + HNO3 (aq) If 20.0…

A: Given: Mass of HCl=20.0 g Mass of HgNO3=30.0 g Percentage yield=78.4% To find: Reagent in excess…

Q: 6. Calculate the stoichiometric formula of a compound, which is defined by the mass composition: C:…

A: The question is based on elemental chemistry. We need to calculate empirical formula of the given…

Q: Gases are sold in large cylinders at high pressure for laboratory use. If a 40.0 L cylinder of…

A: Given :- Pressure = 735 psi Volume = 40.0 L Temperature = 22°C To calculate :- No.of O2…

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

100%

Percent Composition from a Chemical Formula
The percent composition of a compound can also be determined from the formula of the
compound. The subscripts in the formula are first used to calculate the mass of each element in
one mole of the compound. That is divided by the molar mass of the compound and multiplied
by 100%100%.
mass of element in 1 mol
% by mass =
x 100%
molar mass of compound
Step by Step
Calculation of Percent
Composition of a compound
Example:
A certain newly synthesized compound is known to contain the elements zinc and oxygen. When
a 20.00g20.00g sample of the compound is decomposed, 16.07gof zinc remains. Determine the
percent composition of the compound.
Step 1: List the known quantities and plan the problem.
Known
Mass of compound =20.00g
Mass of Zn=16.07gZn
Unknown
Percent Zn=?%
Percent O=?%
Step 2: Subtract to find the mass of oxygen in the compound. Divide each element's mass by the
mass of the compound to find the percent by mass.
Mass of oxygen = 20.00 g – 16.07 g = 3.93 g O
16.07 g Zn
20.00 g
% Zn =
x 100% = 80.35% Zn
3.93 g O
20.00 g
%0 =
x 100% = 19.65% O
Step 3: Conclude the result: The calculations make sense because the sum of the two
percentages adds up to 100%100%. By mass, the compound is mostly zinc.
step 4
Dichlorine heptoxide (Cl207)(Cl207) is a highly reactive compound used in some organic
synthesis reactions. Calculate the percent composition of dichlorine heptoxide. Follow the
step by step procedure shown abo
ve.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider the following measurements then order them from smallest to largest by mass. 0.75 mol H20(liq) 7.0 g N2(g) 0.55 mol Ar(g) 0.45 mol N2(g)
4. How many moles of oxygen are used when 2.22 moles of carbon dioxide are produced? \1_0₂ 6CO₂ + 10 H₂O 2 C3H ₂0 +
Balance the following equation. ___N2H4(g) + ___H2O2(g) → ___N2(g) + ___H2O(g)
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: 2C6H5 Cl + C₂2 HOC13 → C14H9 Cl5 + H₂O chlorobenzene chloral DDT In a government lab, 1167 g of chlorobenzene is reacted with 470 g of chloral. a. What mass of DDT is formed, assuming 100% yield? g b. Which reactant is limiting? Which is in excess? is limiting. Mass= is in excess. c. What mass of the excess reactant is left over? g in excess d. If the actual yield of DDT is 285.0 g, what is the percent yield? Percent yield = % Mass=
1.) Calculate the moles of KHP in flask #1. grams KHP Molar Mass of KHP (A1) 204.22 g/mol moles KHP = 1.224 (A10) %D 204.22 g/mol
Find the number of formula units of CaCI 2 in a 1.5 kg pail of calcium chloride (used to melt Sidewalk ice). [ans: 8.1 X 10 24 formula units]
What number of molecules (or formula units) are present in 2.25 g of each of the following compounds? H a. molecules N b. molecules c. (NH4)2 Cr2O7 formula units
I. Name the two organic compounds. || | GH,0.- C - C-c(CH) -C-C-B Catla Q H 3=0 CH CHIS 0=¢ H CHn. Br
A 14.599 g14.599 g sample of CaCl2CaCl2 was added to 12.147 g12.147 g of K2CO3K2CO3 and mixed in water. A 3.571 g3.571 g yield of CaCO3CaCO3 was obtained. What is the limiting reagent? CaCO3CaCO3 K2CO3K2CO3 CaCl2CaCl2 Calculate the percent yield of CaCO3.CaCO3. yield of CaCO3=CaCO3=
Convert 0.07532 g of C4H10 to molecules.