m/course.html?courseld=16481757&OpenVellumHMAC=feeaec83fa5cc7b2f32454414caf19a1#10001Part CIn the gaseous state, chlorine exists as a diatomic molecule Cl2 (Molar mass = 70.9 g/mol). Calculate the number of moles of chlorine present in 140 g ofchlorine gas.Express the quantity in moles to three significant figures.• View Available Hint(s)?molMoles of chlorine gas =SubmitPrevious AnswersX Incorrect; Try AgainMulti-step problemsA problem that asked you to convert molecules to grams could require two steps1. convert the molecules to molesP Pearson2convert to moles to aremeCopyright O 2021 Pearson Education Inc. All rights reserved. I Terms of Use | Privacy Policy I Permissions | Contact Us |

Answered: Image /qna-images/answer/da9c3dfe-a555-41ff-9580-9441c53e1ce6.jpg

Answered: Part C In the gaseous state, chlorine…

Part C In the gaseous state, chlorine exists as a diatomic molecule Cl2 (Molar mass = 70.9 g/mol). Calculate the number of moles of chlorine present in 140 g of chlorine gas.

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: Calculate, to the correct number of significant figures, how many molecules of Sg are contained in…

Q: A flask contains 0.470 mol of liquid bromine, Br2. Determine the number of bromine molecules present…

A: It is given that there is 0.470 mol of liquid bromine.

Q: The compound known as butylated hydroxytoluene, abbreviated as BHT, contains carbon, hydrogen, and…

A: Consider the given information is as follows; Mass of sample = 3.751 g Mass of CO2 = 11.24 g Mass of…

Q: need

A: We will use stoichiometry of the reaction

Q: Consider the chemical formula for one molecule of methane, CH4. If instead of one molecule we had 10…

A: According to chemical formula of methane ( CH4 ) , it's very clear each molecule of methane has one…

Q: Combustion of a hydrocarbon in a limited supply of air produces COCO in addition to CO2CO2 and…

A: You don't provide the amount of water. But based on my experience put this value. If this value is…

Q: A flask contains 0.390 mol of liquid bromine, Br2. Determine the number of bromine molecules present…

A: Given, Number of moles = 0.390

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: Hydrogen peroxide ( H 2 O 2 ) decomposes to produce water and oxygen.Write a balanced chemical…

A: BALANCED EQUATION IS BELOW :

Q: Fermentation is a complex chemical process of wine making in which glucose is converted into ethanol…

Q: un o 8u described in this laboratory. After heating, the sample is found to weigh 2.245 grams. How…

Q: How many molecules are in 4.83×1020 H2O2? I don't quite understand how to do these calculations. I…

A: Note: Hey there! Thank you for posting the question. Since the unit is not given, we have taken…

Q: A candle flame produces easily seen specks of soot near the edges of the flame, especially when the…

A: Empirical formula: The simplest positive integer ratio of atoms present in a compound is known as…

Q: 1. The organic solvent thiophene is a carbon-hydrogen-sulfur compound that yields CO2, H2O, and SO2…

A: Given: Mass of compound burned = 1.3020 g. Mass of CO2 produced = 2.7224 g. Mass of H2O produced =…

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: According to the following reaction, how many moles of chlorine gas are necessary to form 0.452…

Q: How many moles are represented by 3.65x10^34 molecules of water?

A: Given: molecules of water = 3.65×1034

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

Q: Aluminium has a density of 2.70 | g/cm3 . How many moles of aluminum are in a 13.2 cm3 block of the…

A: Density :- Density of a substance is its amountof mass per unit volume . So , density is the…

Q: Convert 5.17 x 10-22 grams of X5Z2 into molecules/formula units of the same compound. (Assume that…

A: Mass of X5Z2 =5.17 x 10-22 g Molar mass of X =38.46 g/mol Molar mass of Z= 6.17 g/mol Molar mass of…

Q: Elemental S reacts with O₂ to form SO3 according to the reaction 2S+302-2SO3 as depicted here. How…

Q: Ammonium perchlorate NH4ClO4 is the solid rocket fuel that was used by the U.S. Space Shuttle and is…

A: The objective of this question is to determine the mass of water produced by the reaction of 6.89g…

Q: Assuming complete reaction, how many moles of HCl(g) can be produced from 0.100 mol of Cl2(g)?

A: H2(g) + Cl2(g) ----> 2HCl(g) given :- 0.100 mol Cl2(g) To calculate :- number of moles of…

Q: Write the balanced equation: White phosphorus, P4, burns in air to form a compound with a mass…

A: Given that White phosphorus, P4, burns in air to form a compound with a mass percentage composition…

Q: A given sample of Xenon flouride compound contains molecules of the same type XeFn where n is some…

A: Chemical formula which shows number of chemical elements and total element’s number available in…

Q: Calculate the molar mass of lead(II) nitrate, Pb(NO3)2(s)

A: The molar mass is the sum of masses of all the atoms present in compound.

Q: If a sample of B10H12[N(CH3)3]2 is found to contain 7.48 · 1020 B atoms how many N atoms are…

A: Given: number of B atoms = 7.48×1020 atoms

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: 1)Copper metal reacts with molecular nitrogen to form copper(II) nitride. a)Write the balanced…

Q: In a first expirement, a compound is analyzed and found to contain 85.63% C and 14.37% hydrogen by…

A: 1. atom % in samp;e mole Mole ratio (divided by smallest number of moles) C 85.63 85.63 /12 =…

Q: Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 20.0 g…

A: The balanced reaction taking place is N2O4 (l) + 2 N2H4 (l) → 3 N2 (g) + 4 H2O (g) Given : mass of…

Q: Use the References to access important values If needed for this question. For the molecular…

A: In this question we have to convert mole into molecule by some multiply.

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

m/course.html?courseld=16481757&OpenVellumHMAC=feeaec83fa5cc7b2f32454414caf19a1#10001
Part C
In the gaseous state, chlorine exists as a diatomic molecule Cl2 (Molar mass = 70.9 g/mol). Calculate the number of moles of chlorine present in 140 g of
chlorine gas.
Express the quantity in moles to three significant figures.
• View Available Hint(s)
?
mol
Moles of chlorine gas =
Submit
Previous Answers
X Incorrect; Try Again
Multi-step problems
A problem that asked you to convert molecules to grams could require two steps
1. convert the molecules to moles
P Pearson
2convert to moles to areme
Copyright O 2021 Pearson Education Inc. All rights reserved. I Terms of Use | Privacy Policy I Permissions | Contact Us |

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

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

See the example in Introduction for set-up of calculations. Calculate the number of a) moles of F b) atoms of F in 32.5 g of fluorine gas, F 2 .
organic solvent) that contains 1.00 x 1012 molecules 2. Calculate the mass of chloroform (CHC13, an of chloroform.
General Chemistry 4th Edition University Science Books presented by Macmillan Learning McQuarrie • Rock • Gallogly A hydrated form of copper sulfate (CUSO, · xH, 0) is heated to drive off all of the water. If there is initially 9.94 g of hydrated salt and there is 6.35 g of anhydrous CUSO, after heating, find the number of water molecules associated with each CUSO, formula unit. X =
calculate the number of molecules in 0.256 g of NH4Cl. (molar mass of NH4Cl = 53.492 g/mol; 1 mole = 6.02x10^23)
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.
Calculate the mass (in kilograms) of chlorine in 25 kg of chlorofluorocarbon (CFC). CF3Cl
Convert 5.42 x 10-21 grams of X3Z5 into molecules/formula units of the same compound. (Assume that the molar mass of X is 72.13 grams per mole and the molar mass of Z is 79.81 grams per mole.) Assume that Avogadro's number is 6.022 x 1023. Report your answer to three decimal places.
43. One of the ingredients in the Native American stomachache remedy derived from common chokecherry is caffeic acid which is comprised of carbon, hydrogen, and oxygen only. Combustion of 1.00  102 mg of caffeic acid yielded 220 mg of CO2 and 40.3 mg of H2O. Determine the empirical formula of caffeic acid. You may check your answer by looking up the answer, but do not use the formula to solve the problem.