Pleeesssseeee solve quuuuuuestion 4 3.4.Calculate the percent composition of each elementof formaldehyde (CH2O).Benzene has the following percent compositions:92.31% of Carbon and 7.69 % of Hydrogen. Whatis the empirical formula for Benzene?5. A compound with an empirical formula of SNH.Determine its molecular formula, given that itstrue molar mass is 188.35 g/mol

In the given question we have to determine the empirical formula of benzene, First, we have to…

Answered: 3. 4. Calculate the percent composition…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter11: Stoichiometry

Section: Chapter Questions

Problem 115A

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hat is the difference between the empirical and molecular for mulas of a compound? Can they ever be the same? Explain.
Copper(I) iodide (CuI) is often added to table salt as a dietary source of iodine. How many moles of CuI Are contained in 1.00 lb (454 g) of table salt containing 0.0100% CuI by mass?
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
When small quantities of elemental hydrogen gas are needed for laboratory work, the hydrogen is often generated by chemical reaction of a metal with acid. For example, tine reacts with hydrochloric acid, releasing gaseous elemental hydrogen: :math>Zn(s)+2HCI(aq)ZnCl2(aq)+H2(g) at mass of hydrogen gas is produced when 2.50 g of zinc is reacted with excess aqueous hydrochloride acid?
Consider the following diagram, where atom X is represented by a square and atom Y is represented by a circle. (a) Write the equation for the reaction represented by the diagram. (b) If each circle stands for a mole of Y and each square a mole of X, how many moles of X did one start with? How many moles of Y? (c) Using the same representation described in part (b), how many moles of product are formed? How many moles of X and Y are left unreacted?
Cyanogen gas, C2N2, has been found in the gases of outer space. It can react with fluorine to form carbon tetrafluoride and nitrogen trifluoride. C2N2(g)+7F2(g)2CF4(g)+2NF3(g)(a) How many moles of fluorine react with 1.37 mol of cyanogen? (b) How many moles of CF4 are obtained from 13.75 mol of fluorine? (c) How many moles of cyanogen are required to produce 0.8974 mol of NF3? (d) How many moles of fluorine will yield 4.981 mol of nitrogen trifluoride?
The active ingredient in aspirin is acetylsalicylic acid, which has the chemical formula C9H8O4. An aspirin pill contains 300.0 mg of acetylsalicylic acid. How many moles of acetylsalicylic acid does it contain?
PERCENT COMPOSITION AND EMPIRICAL FORMULA OF A HYDRATE Partial empirical formula of the hydrate used: CoCl2 • -----> H2O Mass of empty beaker + watch glass: 154.00g Mass of beaker and hydrate (before heating): 155.58g Mass of beaker and anhydrous salt (after heating): 154.72g A. Show the calculations for determining the mass of the hydrate used: B. Show the calculations for determining the mass of anhydrous salt produced: C. Show the calculations for determining the mass of water in the original hydrate: D. Show the calculations for determining the expirimental percent of water in the hydrate:
Cinnamic alcohol is used mainly in perfumery, particularly in soaps and cosmetics. Its molecular formula is C,H₁0O. / Part 1 of 2 Calculate the percent composition by mass of C, H, and O in cinnamic alcohol. % C Part 2 of 2 % H % O Round your answers to 2 decimal places. X How many molecules of cinnamic alcohol are contained in a 0.836 g sample? molecules x10
A compound is 40.0% C, 6.70% H, and 53.3% O by mass. Assume that we have a 100.-g sample of this compound. What are the subscripts in the empirical formula of this compound? Enter the subscripts for C, H, and O, respectively, separated by commas (e.g., 5,6,7). Worj this out step by step so i can better understand.
wo Cerme uY 5. How many grams of Na are in 0.576 mol Na? 6. How many moles of calcium chloride are in 2.25 x 10 molecules of calcium chloride? 7. Analysis of a popular food flavor is determined to be 35.5% C, 4.77% H, 8.29% N, 13.6% Na, and 37.9% O. What is its empirical formula?
5. Aspartame is an artificial sweetener that is 160 times sweeter than sucrose (table sugar) when dissolved in water. It is marketed as Nutra-Sweet. The molecular formula of aspartame is C14H18N2O5. Calculate the following a. Molar mass of aspartame b. What amount of molecules are present in 10.0 g aspartame c. The mass in grams of 1.56 mol aspartame d. What number of molecules are in 5.0 mg aspartame e. What number of atoms of nitrogen are in 1.2 g aspartame f. What is the mass in grams of 1.0 x 109 molecules of aspartame g. What is the mass in grams of one molecule of aspartame

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