226.compound.lomso lealto i ba readin AThe mass percent of water in a hydrate of MnCl, is 36.41%. What is the empirical formula ofthe hydrate?7.8.* A 4.00 gram sample of a hydrate of nickel(II) bromide loses 0.793 grams of water when heated.Determine the mass percent water in the hydrate and the formula of the hydrate.a gnininoo to colbe ts anoonis laubn olaodlo eaM 89. A 2.500 gram sample of a hydrate of calcium sulfate loses 0.523 grams of water when heated.Determine the mass percent of water in the hydrate and the formula of the hydrate.01bbolobiboi10. An unknown solution containing one of the salts ZnSO4, MgSO, or SrCl, gives a negative flametest but tarnishes a piece of magnesium inserted into the solution. Which salt was in thesolution?11. The heating of CuSO,· 5H,O yields several transitions as a function of temperature. The tablebelow gives the percentage of original mass lost as a function of the approximate temperature.Use these percentages to determine the sequence of decompositions and write chemicalequations for each transition.percentage of original mass lostapproximate temperature (°C)14.529.036.051.567.070.51001302208009101020 oMboanis to oO 2015 Cengage Leaming. All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly accessible website, in whole or in part.

Given : 40% carbon, 6.71% Hydrogen and 53.29% Oxygen. To find : Empirical formula and molecular…

Answered: 22 is -o ben ealua9 l b ade A compound.…

Science

Chemistry

22 is -o ben ealua9 l b ade A compound. lomy

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 191IP: With the advent of techniques such as scanning tunneling microscopy, it is now possible to write...

See similar textbooks

Similar questions

A binary compound of magnesium and nitrogen is analyzed, and 1.2791 g of the compound ¡s found to contain 0.9240 g of magnesium. When a second sample of this compound is treated with water and heated, the nitrogen is driven off as ammonia, leaving a compound that contains 60.31% magnesium and 39.69% oxygen by mass. Calculate the empirical formulas of the two magnesium compounds.
A sample of an oxide of vanadium weighing 4.589 g was heated with hydrogen gas to form water and another oxide of vanadium weighing 3.782 g. The second oxide was treated further with hydrogen until only 2.573 g of vanadium metal remained. (a) What are the simplest formulas of the two oxides? (b) What is the total mass of water formed in the successive reactions?
Fulgurites are the products of the melting that occurs when lightning strikes the earth. Microscopic examination of a sand fulgurite shows that it is a globule with variable composition that contains some grains of the definite chemical composition Fe 46.01%, Si 53.99%. Determine the empirical formula of these grains.
The empirical formula of a gaseous fluorocarbon is CF2 . At a certain temperature and pressure, a 1-L volume holds 8.93 g of this fluorocarbon, whereas under the same conditions, the 1-L volume holds only 1.70 g gaseous fluorine (F2) . Determine the molecular formula of this compound.
It sodium peroxide is added to water, elemental oxygen gas is generated: :math>Na2O2(s)+H2O(l)NaOH(aq)+O2(g) ppose 3.25 g of sodium peroxide is added to a large excess of water. What mass of oxygen gas will be produced?
Hexachlorophene, a compound made up of atoms of carbon, hydrogen, chlorine, and oxygen, is an ingredient in germicidal soaps. Combustion of a 1.000-g sample yields 1.407 g of carbon dioxide, 0.134 g of water, and 0.523 g of chlorine gas. What are the mass percents of carbon, hydrogen, oxygen, and chlorine in hexachlorophene?
When 9.59 g of a certain vanadium oxide is heated in the presence of hydrogen, and a new oxide of vanadium are formed. This new vanadium oxide has a mass of 8.76 g. When the second vanadium oxide undergoes additional heating in the presence Of hydrogen, 5.38 g of vanadium metal forms, a. Determine the empirical formulas for the two vanadium oxides. b. Write balanced equations for the Steps of the reaction. c. Determine the mass of hydrogen needed to complete the steps of this reaction.
A 0.755-g sample of hydrated copper(II) sulfate CuSo4xH2O was heated carefully until it had changed completely to anhydrous copper(II) sulfate (CuSO4 ) with a mass of 0.4183 g. Determine the value of x. [This number is called the number of waters of hydration of copper(II) sulfate. It specifies the number of water molecules per formula unit ofCuSO4 in the hydrated crystal.]
An air bag is deployed by utilizing the following re tion the nitrogen gas produced inflates the air bag): :math>2NaN3(s)2Na(s)+3N2(g) 10.5 g of NaN1 is decomposed, what theoretical mass of sodium should be produced? If only 2.84 g of sodium is actually collected, what is the percent yield?
A jar contains some number of jelly beans. To find out precisely how many are in the jar, you could dump them out and count them. How could you estimate their number without counting each one? (Chemists need to do just this kind of bean counting when they work with atoms and molecules. Atoms and molecules are too small to count one by one, so chemists have worked out other methods to determine the number of atoms in a sample.)
A chemist prepared a compound that she thought had the formula FeI3. When the compound was analyzed, it contained 18.0% Fe and 82.0% I. Calculate the mass percentage composition expected for FeI3 and compare the result with that found in the analysis. Is this the correct formula of the compound?
Suppose Avogadro’s number was 1000 instead of 6.0221023 . How, if at all, would this affect the relative masses on the periodic table? How, if at all, would this affect the absolute masses of the elements?