A sample of hydrocarbon on complete combustion gave 1.32 g of carbon dioxide and 0.72 g of water. What would be the empirical formula of the hydrocarbon giv the following relative atomic masses: H = 1.0; C= 12.0 4. A CH2 B C3H4 C;Hs

A sample of hydrocarbon on complete combustion gave 1.32 g of carbon dioxide and 0.72 g of water. What would be the empirical formula of the hydrocarbon giv the following relative atomic masses: H = 1.0; C= 12.0 4. A CH2 B C3H4 C;Hs

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

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 171CP: Consider the following data for three binary compounds of hydrogen and nitrogen: %H (by Mass) %N...

See similar textbooks

Related questions

Q: Vhich molecular formula is also an empirical formula? O H202 O C6H1206 C2H4 PCI3

A: It’s explained below:

Q: A 0.370-mol sample of a metal oxide (M₂O₃) weighs 55.4 g.(a) How many moles of O are in the…

A: Mass of 0.37 mole of metal oxide = 55.4 g. Mass of one mole of metal oxide = Molar mass of the metal…

Q: Citric acid was found to contain 37.51% C, 4.20% H, and 58.29% O by mass. What is the simplest…

A: Given :- Percent composition of C = 37.51% Percent composition of H = 4.20% Percent composition…

Q: Eucalyptus leaves are the food source for panda bears. Eucalyptol is an oilfound in these leaves.…

Q: (a) The characteristic odor of pineapple is due to ethyl butyrate,a compound containing carbon,…

Q: Q) 5 The complete combustion of 0.1 g of menthol produces 0.282 g of CO, and 0.115 g of H,O…

A: To find the empirical formula of the menthol, moles of carbon, hydrogen and oxygen need to be…

Q: What is the molecular formula of a compound with the empirical formula CH2CH2 and a formula mass of…

A: Empirical formula of compound=CH2 Mass of empirical formula=1 x atomic mass of C + 2 x atomic mass…

Q: 2. The foul odor of rancid butter is due largely to butyric acid, a compound containing carbon,…

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

Q: wnat is the empiracle formula og Compound that is 62.07. C, 10.47 and 27.5%. 0 by mass ?

A: C = 62.0 % H = 10.4 % O = 27.5 %

Q: A compound has the empirical formula C6H7N and a formula mass of 186.24 g/mol. What is the molecular…

A: Answer: Option d. C12H14N2 is the correct molecular formula. Given,The empirical formula=C6H7N…

Q: A compound has the empirical formula CH20 and a formula mass of 120.10 g/mol. What is the molecular…

A: Given empirical formula ⇒ CH2O Formula mass = 120.10 g/mol Molecular mass =…

Q: 1. An organic compound with a molar mass of 183.18 g/mol has the following mass percents ol each…

A: An organic compound is having molar mass = 183.18 g/mol Portion of Carbon = 39.34 % of 183.18 = 72…

Q: Caffeine, a stimulant in coffee and tea, a molar mass of 194.19 g/mol and a mass percentage…

A: Given,

Q: A 0.370-mol sample of a metal oxide (M2O3) weighs 55.4 g. (a) How many moles of O are in the sample?…

A: A 0.370-mol sample of a metal oxide (M2O3) weighs 55.4 g. (a) How many moles of O are in the sample?…

Q: H2lg) reacts with N{g) to produce NH3(g). What mass of H2(g) is required toct completely and produce…

Q: 0.1890 gm of a compound gave on combustion 0.1761 gm of CO2 and 0.0540 gm of H2O. Its molecular mass…

Q: 3. Calculate the percentage by mass of oxygen in the following compounds: (#3.25, p.157) a.…

A: formula for percentage by mass:

Q: A hydrocarbon (i.e. with only carbon and hydrogen) is combusted with excess oxygen to produce 352 g…

A: The simplest notation of any compound is its empirical formula that outlines the elements' ratio…

Q: 3. Calculate the percentage by mass of oxygen in the following compounds: (#3.25, p.157) a.…

A: Vanillin ---- molecular formula -12×8+1×8+16×3=152 (atomic mass of oxygen…

Q: Which is an empirical formula? O C2H6 O C6H6 O C3 Hg O C4 Hg

A: For the 1st question: Given formulas: C2H6, C6H6, C3H8, C4H8 We have to find out which one of them…

Q: In an experiment, 2.7g of compound C yielded 1.48g of C6H5CH2OCH2C6H5. What is the percentage yield?…

Q: Given the reaction below, if 3.64 moles of Vanadium (V) were reacted with 4.88 moles of Oxygen (O2)…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: (a) Combustion analysis of toluene, a common organicsolvent, gives 5.86 mg of CO2 and 1.37 mg of…

A: (a) The number of moles of C and H present in the hydrocarbon can be calculated using the mass of…

Q: The empirical formulae and molar masses of three compounds, A, B and C, are shown in Table 3.7.…

A: Empirical formula :- The chemical formula which shows only the relative number of atoms of…

Q: A molecule has an empirical formula of Ch2. 1.34 moles of the compound give 530.76 g of CO2 upon…

A: Given : We have to calculate the molecular formula.

Q: Calculate the Molar mass of the following: 1. C14H29NO4S ( Penicillin – an antibiotic) 2.…

A: The molar mass or molecular weight of any compound is the sum of the mass of each element present in…

Q: The compound dioxane, which is used as a solvent in variousindustrial processes, is composed of C,…

A: Molar mass of the given compound is 88.1 g/mol.

Q: 3.1. How many moles and how many molecules are there in 750g of a) H2 b) H2O c) H2SO4? How many…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: 32. The empirical formula of a compound is CH,O. If 0.0832 mole of the compound contains 1.0 g of…

A: Empirical formula of compound is [CH2O]X 0.0835 mole of compound contains 1g of hydrogen1 mole of…

Q: moles of water combined with 1 mole of KAl(SO4)2, and the formula of the hydrate

A: A compound which has the capacity of to hold water of crystallisation is known as hydrated salt a…

Q: Nicotine, a component of tobacco, is composed of C, H and N. A 5.20-mg sample of nicotine was…

Q: Given the reaction below, if 3.64 moles of Vanadium (V) were reacted with 4.88 moles of Oxygen (O2)…

A: First see the mol ratio of V and O2 from the reaction , and apply it for the reaction.

Q: The winds in a hurricane can travel as high as 200.0 miles per hour. What is this speed in meters…

Q: What is the molecular formula of a compound with a percent composition of 49.47% C, 5.201% H, 28.84%…

A: The given data contains, Carbon =49.47% Hydrogen =5.201% Nitrogen =28.84% Oxygen =16.48 %

Q: 3. a. If "Epsom salt", MgSO4. xH₂O, is heated to 250 ° C, all the water of hydration is lost. Write…

A: Epsom salt = MgSO4. xH2O xH2O is the water of crystallization attached physically to the salt. a)…

Q: (a) The molecular formula of acetylsalicylic acid (aspirin),one of the most common pain relievers,…

A: a) Since the molar mass of aspirin = Atomic mass of C X 9 + Atomic mass of H X 8 + Atomic mass of O…

Q: Which of the following is not an empirical formula C2H6 C2H CH3 CH

A: We are having the four different formulas of certain compound. We have to see which formula is not…

Q: A Freon™ leak in the air conditioning system of an old car releases 25g of CF2Cl2 per month. What…

A: 25 g of CF2Cl2 is released by an old car air conditioning system per month.

Q: A compound has the empirical formula C3H4N. The molar mass of the compound is 108.16 g/mol. What is…

A: Given, Empirical formula : C3H4N Molar mass = 108.16 g/mol Molecular Formula = ?

Q: The molecular formula of aspartame, the artificial sweetenermarketed as NutraSweet®, is C14H18N2O5.…

A: Aspartame is an artificial sweetener that is 200 times sweeter than the sucrose is marketed as…

Q: Without doing any detailed calculations (but using a periodic table to give atomic weights), rank…

A: Each mole of any molecule contains Avogadro no of molecules i.e 6.023x10^23. It is true for every…

Q: hat number of molecules (or formula units) are present in 1.69 g of each of the following compounds…

A: Find the number of moles of each and multiply each number of moles with avagadro number. Number of…

Q: In order to determine the formula of CoCl.xH;O, a student heated 0.476 g of hydrate. The mass of…

A: First of all we have to calculate the weight of water that goes off after being heated. Convert…

Q: A compound consists of 85.7%C and 14.3% H . Its molar mass is 42.0g. How do I find its molecular…

A: empirical formula : Simplest positive integer ratio of atoms present in a compound Given Carbon…

Q: C. An organic compound, in liquid form, comprises of 59.2% C, 13.6% H and and has a molar mass of 60…

Q: What is the formula weight of the compound Al2(SO4)3*18H2O?

A: To calculate the formula weight of the given compound, Al2(SO4)3*18H2O, we need to know the molar…

Concept explainers

Mass Spectrometry

This process is an instrumental method in which a sample is changed to fast moving positive ions by electron bombardment. The charged particles vary due to their different mass to charge ratio and are estimated with the help of this difference. It is also called mass spectroscopy.

Question

A sample of hydrocarbon on complete
combustion gave 1.32 g of carbon dioxide
and 0.72 g of water. What would be the
empirical formula of the hydrocarbon given
the following relative atomic masses:
H = 1.0; C= 12.0
4.
A
CH2
B
C3H4
C;Hs
D

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 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

A compound associated with the odor of garlic on a persons breath has the chemical formula CyH8S and a formula mass of 88.19 amu. What number does y stand for in the chemical formula of the compound?
By x-ray diffraction it is possible to determine the geometric pattern in which atoms are arranged in a crystal and the distances between atoms. In a crystal of silver, four atoms effectively occupy the volume of a cube 0.409 nm on an edge. Taking the density of silver to be 10.5 g/cm3, calculate the number of atoms in one mole of silver.
The compound 1-propanethiol, which is the eye irritant released when fresh onions are chopped up, has the chemical formula C3HyS and a formula mass of 76.18 amu. What number does y stand for in the chemical formula of the compound?
Consider the following data for three binary compounds of hydrogen and nitrogen: %H (by Mass) %N (by Mass) I 17.75 82.25 II 12.58 87.42 III 2.34 97.66 When 1.00 L of each gaseous compound is decomposed to its elements, the following volumes of H2(g) and N2(g) are obtained: H2(L) N2(L) I 1.50 0.50 II 2.00 1.00 III 0.50 1.50 Use these data to determine the molecular formulas of compounds I, II, and III and to determine the relative values for the atomic masses of hydrogen and nitrogen.
The element bromine is Br2, so the mass of a Br2 molecule is the sum of the mass of its two atoms. Bromine has two isotopes. The mass spectrum of Br2 produces three peaks with relative masses of 157.836, 159.834, and 161.832, and relative heights of 6.337, 12.499. and 6.164, respectively. (a) What isotopes of bromine are present in each of the three peaks? (b) What is the mass of each bromine isotope? (c) What is the average atomic mass of bromine? (d) What is the abundance of each of the two bromine isotopes?
Two basic laws of chemistry are the law of conservation of mass and the law of constant composition. Which of these laws (if any) do the following statements illustrate? (a) Lavoisier found that when mercury(ll) oxide, HgO, decomposes, the total mass of mercury (Hg) and oxygen formed equals the mass of mercury(ll) oxide decomposed. (b) Analysis of the calcium carbonate found in the marble mined in Carrara, Italy, and in the stalactites of the Carlsbad Caverns in New Mexico gives the same value for the percentage of calcium in calcium carbonate. (c) Hydrogen occurs as a mixture of two isotopes, one of which is twice as heavy as the other.
Determine the molecular mass of the following compounds:
Cyclopropane is an interesting hydrocarbon. Instead of havingthree carbons in a row, the three carbons form a ring, asshown in this perspective drawing (see Figure 2.18 for a priorexample of this kind of drawing): Cyclopropane was at one time used as an anesthetic, but its use was discontinued, in part because it is highly flammable.(a) What is the empirical formula of cyclopropane? Howdoes it differ from that of propane? (b) The three carbon atomsare necessarily in a plane. What do the different wedgesmean? (c) What change would you make to the structureshown to illustrate chlorocyclopropane? Are there isomers ofchlorocyclopropane?
Cyclopropane is an interesting hydrocarbon. Instead of havingthree carbons in a row, the three carbons form a ring, asshown in this perspective drawing (see Figure 2.18 for a priorexample of this kind of drawing):Cyclopropane was at one time used as an anesthetic, but itsuse was discontinued, in part because it is highly flammable.(a) What is the empirical formula of cyclopropane? Howdoes it differ from that of propane? (b) The three carbon atomsare necessarily in a plane. What do the different wedgesmean? (c) What change would you make to the structureshown to illustrate chlorocyclopropane? Are there isomers ofchlorocyclopropane?
How many carbon atoms are in 29 molecules of benzene, C₆H₆?
ow many moles of H2O does 1.2 x 1024 molecules represent?
What is the mass of 5.83 ×1017 molecules of liquid propane, C3H8?