Answered: The percent composition by mass of an…

The percent composition by mass of an unknown chlorinated hydrocarbon was found to be 37.83%C, 6.35%H, and 55.83%Cl by mass. What is the empirical?

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: The first step in the manufacture of nitric acid by the Ostwald process is the reaction of ammonia…

A: Limiting reagent is the reagent which is consumed in the chemical reaction completely. It decides…

Q: hen copper is heated with an excess of sulfur, copper(I) sulfide is formed. In a given experiment,…

Q: acrylic acid used in the manufacture of acrylic plastics has the composition 50.%C 5.6%H and 44.4%O…

Q: If 6.1 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, what is the mass in kg of CO₂…

A: Given: 6.1 × 10²⁵ molecules of CO₂ are produced in a combustion reaction. To determine : The mass…

Q: Malonic acid is used in the manufacture of barbiturates (sleeping pills). The composition of the…

A: To calculate the mole of each elements present in Malonic acid: Given: 34.56 % of C, 3.9 % of H, and…

Q: Allí in a potent antibacterial compound, is formed by the enzyme allinase when garlic is chopped or…

A: Allí compounds contains four atom carbon, Hydrogen, Oxygen, Sulfur 10 mg produced Alli 16.27 mg…

Q: The foul odor of rancid butter is due largely to to butyric acid, a compound containing carbon,…

A: 1) Given, Butyric acid, a compound containing carbon, hydrogen, and oxygen. mass of sample = 4.30 g…

Q: A certain compound, used as a welding fuel, contains only carbon and hydrogen. Burning a small…

Q: 3. In determining the simplest formula of lead sulfide, 2.46grams of lead are placed in a crucible…

A: The mass of the lead is 2.46 g.The mass of the product is 3.22 g.

Q: A certain gasoline additive that boosts the octane rating of gasoline is made of the elements C, H,…

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: 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: The synthesis of maleic acid anhydride (C₄H₂O₃) can be accomplished by reacting benzene (C₆H₆) and…

A: We have, actual yield of maleic acid anhydride = 128.3 g and, percent yield = 72.6 % We…

Q: What mass of iron (III) oxide is produced when 3.88 X 1025 grams of oxygen reacts with excess…

Q: Ascorbic acid is one form of vitamin C and is known to contain only carbon, hydrogen, and oxygen.…

A: Given, The mass percent of Carbon = 40.91% Hydrogen = 4.578% and Oxygen = 54.50% The mass of the…

Q: [References] A sample of limestone and other soil materials was heated, and the limestone decomposed…

A: Calcium carbonate decomposes into calcium oxide and carbon dioxide. The equation for the balanced…

Q: A sample of a substance with the empirical formula XCI3 weighs 0.4884 g. When it is dissolved in…

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

Q: The reaction of 7.71 x 103 g of titanium (IV) chloride gas with 1.45 x 103 g of oxygen gas produces…

A: Titanium chloride reacts with oxygen to give titanium oxide and two moles of chlorine gas.

Q: The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many…

Q: A student obtains a mixture of the chlorides of two unknown metals, X and Z. The percent by mass of…

A: Given: Mixture of metal X and Z. And mass percent of X and Z in the mixture.

Q: A compound of copper was formed when 1.643 g of Cu was heated in oxygen. The mass of the compound…

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 1.000 g sample of an unknown compound containing only carbon, hydrogen, and oxygen was analyzed…

A: Given: Mass of sample = 1.000 g Mass of CO2 formed = 2.579 g Mass of H₂O formed = 0.6536 g Molar…

Q: If 2.332 g of a sample containing a mixture of CuO and CuCO3 are heated, the final weight of the…

A: CuCO3 on heating decomposes to form CuO and CO2 CuCO3 (s) →heat CuO (s) + CO2 (g) 123.55 g…

Q: Compound X has a molar mass of 176.12·gmol−1 and the following composition: element mass % carbon…

Q: A 1.000 g sample of an unknown compound containing only carbon, hydrogen, and oxygen was analyzed…

Q: The empirical formula of a compound is CH2O and its formula weight is 120.12 amu. What is the…

Q: The synthesis of maleic acid anhydride (C₄H₂O₃) can be accomplished by reacting benzene (C₆H₆) and…

A: 2 C₆H₆(l) + 9 O₂(g) → 2 C₄H₂O₃(s) + 4 CO₂(g) + 4 H₂O(g)According to the above equation, 9 moles of…

Q: empirical formula of bismuth chloride?

Q: What mass of iron (III) oxide is produced

A: Number of moles = mass/molar mass Molar mass of O2 = 31.999 g/mol Molar mass of iron (iii) oxide =…

Q: How many moles (of molecules or formula units) are in each sample? 0.2011 g C8H18 Express your…

A: Given, mass of C8H18 = 0.2011 g Molar mass of C8H18 = 114.23 g/mol

Q: Minerals in soils and soil amendments (e.g., fertilizers) are described by formula units that…

A: To calculate: What is the mass in grams of 0.518 moles of calcium carbonate (CaCO3)?

Q: 328.8 g SO2(g), 425.3 g CaCO3(s), and 105.7 g 02(g) react as follows: 2 SO2(g) + 2 CaCO3 (s) + 02(g)…

A: Mass of SO2= 328.8 g Mass of CaCO3= 425.3 g Mass of O2=105.7 g

Q: A certain organic acid contains 26.68 % carbon, 2.24 % hydrogen, and 71.08% oxygen by mass. A 0.050…

Q: If 0.100 g of a compound containing C, H, and O is combusted completed in an excess of oxygen and…

A: Mass of the Carbon can be calculated as

Q: Calculate the mass percent of carbon in glucose (C6H12O6).

A: Dear student, since you have asked multiple questions but according to guidelines we will solve 1st…

Q: When a sample of acetic acid (vinegar) is burned, it can be determined that it has a mass percentage…

A: Given: Mass percentage of Carbon =39.9% Mass percentage of Hydrogen =6.72% Mass percentage of…

Q: One medication used to treat diabetic kidney disease, high blood pressure, and heart failure is made…

Q: Caffeine, an extremely popular chemical amongst students and teachers alike, is composed of four…

A: Given, carbon 49.48 % hydrogen 5.19 % nitrogen 28.85 % oxygen 16.48 %

Q: A student synthesizes tin oxide to create a compound with generic formula SnxOy. She does this by…

A: Given : mass of product = 39.10 g Mass of oxygen= 30.80 g Molar mass of oxygen= 15.999…

Q: calculate the fraction of methane in the mixture.

A: Given: The mass of mixture of methane CH4 and ethane C2H6=13.43 g The total mass of CO2 and…

Q: A student determined the mass of NaCl extracted during an experiment to be 0.42 grams. If the mass…

A: Given Mass of NaCl = 0.42 g Mass of original mixture = 1.97 g

Q: When 5.762 g of a compound composed of only carbon, hydrogen, and oxygen was submitted to combustion…

Question

The percent composition by mass of an unknown chlorinated hydrocarbon was found to be 37.83%C, 6.35%H, and 55.83%Cl by mass. What is the empirical?

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Consider the copper thermite reaction, a reaction between two solids that can be initiated with strong heating: 3 CuO(s) + 2 Al(s) → 3 Cu(s) + Al2O3(s) 25.0 g of copper(II) oxide are combined with 25.0 g of Al , and the mixture is heated strongly to react. molar masses (g/mol): CuO - 79.55 Al - 26.98 Cu - 63.55 What is the chemical formula or elemental symbol for the limiting reactant? What is the chemical formula or elemental symbol for the excess reactant?
Nitesh
If 226.1 g of tin(II) chloride was the actual amount obtained in a reaction for which the theoretical yield was 288.0 g, the percentage yield is what?
What mass of iron (III) oxide is produced when 3.88 X 1025 grams of oxygen reacts with excess iron?
In an experiment to determine the empirical formula of magnesium chloride, 0.50 g of magnesium ribbon was taken in a beaker and a few drops of HCl was added until all the Mg reacted with the acid liberating the hydrogen gas. The reaction completion was noted by observing that the bubbling stopped and no solid Mg was seen in the beaker. The beaker was heated to remove water and the dried magnesium chloride was weighed and found to be 1.99 g. What is the empirical formula for magnesium chloride based on this experiment?
0.333 g of a hydrocarbon (CxHy) was analyzed by combustion analysis and 1.009 g of CO2 (MM = 44.01 g/mol) and 0.516 g of H2O (MM = 18.02 g/mol). How many moles of hydrogen were in the 0.333 g sample? Enter your answer in standard notation to the proper number of significant figures.
An impure sample of table salt (NaCl) that was dissolved in water and treated with silver nitrate to form silver chloride. If the initial sample had a mass of 1.741 g and the final mass of the AgCl was found to be 4.084 g, what is the mass percent of NaCl in the impure sample?
8. An explosive has the following composition by mass: 15.87% Carbon, 2.22% Hydrogen, 18.5% Nitrogen and 63.41% Oxygen. What is the empirical formula of the explosive?
When copper is heated with an excess of sulfur, copper(I) sulfide is formed. In a given experiment, 1.50 g of copper was heated with excess sulfur to yield 1.64 g copper(I) sulfide. What is the percent yield?
When copper is heated with an excess of sulfur, copper(I) sulfide is formed. In a given experiment, 1.50 g of copper was heated with excess sulfur to yield 1.79 g copper(I) sulfide. What is the percent yield?
A compound contains arsenic (As) and oxygen as its only elements. A 1.626 gsample of the compound contains 1.060 g of arsenic.What is the empirical formula for the compound?If the molecular mass is 395.7 g/mol, what is the molecular formula for this compound?
A chemist goes into the lab and performs an experiment in which a mixture of 8.47 grams of Zn and 6.03 g of sulfur are reacted. Before starting the experiment they perform the following calculations to predict the maximum (theoretical) yield of zinc sulfide that could be produced. They obtain an actual yield of 8.25 grams of zinc sulfide. Calculate their percent yield to one decimal place.