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

Step 1:Percent Composition of Formaldehyde (CH2O):To find the percent composition of each element in…

Answered: 3. 4. Calculate the percent composition…

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...

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Q- If iron(lll) phosphate reacts with sodium sulfate to produce iron (lll) sulfate and sodium phosphate the percentage yield of sodium phosphate (Na3PO4)_____ if after the experiment is performed you produce 5.6 grams using 12.7 grams of iron (lll) phosphate?
Fill in the blanks using the other image.
Section 5.9 The Mole and Chemical Equations 11. In the following equations consider the bold formulas. The molar ratio between the two bold formulas can be expressed in two ways. Write them both. a. S(s) + O2(g) → SO2(g) b. Sr(s) + 2H2O(1) → Sr(OH)2(s) + H2(g) c. 4NH3(g) +5O2(g) → 4NO(g) + 6H2O(g) d. CaO(s) + 3C(s) → CaC2(s) +CO(g)
(Record only your final answer rounded to the correct number of significant digits.) 1. The last step in the production of nitric acid is represented by the following reaction: 3 NO2(g) + H2O(l) --> 2 HNO3(aq) + NO(g) Calculate the moles of nitric acid produced when 6.84 mol of nitrogen dioxide react with excess water. 2. In coal, sulfur typically exists in the form of iron pyrites, FeS2, or in organic compounds. Burning coal in power plants converts the sulfur to sulfur dioxide according to the following reaction: 4 FeS2(s) + 11 O2(g) --> 2 Fe2O3(s) + 8 SO2(g) What mass (in grams) of sulfur dioxide is produced when 0.334 mol of oxygen gas reacts?
N2(g) + 3H2(g) → 2NH3(g) Supposed you start with 3.00moles of hydrogen and nitrogen:a. Which would be the limiting reagent?b. How many moles of ammonia would be produced?c. What is the theoretical yield in grams?
Brasses are alloys in which copper is the primary component and zinc is the second most abundant element. Naval brass, which has a high resistance to salt corrosion is 60.0% Cu, 39.25% Zn, and 0.75% Sn. How many moles of zinc are present in a 72.1 gram sample of naval brass? Report your answer with three significant figures.
Molecular Formulas and Percent Composition Name Chem 108 Combustion Analysis molecular compouna containing C, H, N, O 02 gas The sample is combusted CO₂, H₂O, and NO2 are the products of combustion The product mixture is separated and detected % C, %H, %N by mass are reported 1. An unknown compound contains 24.0 % C, 12.0 % H, and some oxygen. Determine its empirical formula. 2. A compound has a molar mass of 160.3 g/mol and its empirical formula is C3H4. What is its molecular formula?
Consider the following reaction: If 19.26 grams of methane reacts with 78.70 grams of chlorine, which reactant is the limiting reagent? CH4(g) + 4 C12(g) CCI4(1) + 4 HCI(g) * Methane, CH4 Chlorine, C12 O Carbon Tetrachloride, CCI4 Hydrogen Chloride, HCI CM that
6
CS2 + 3 Cl2 -> CCl4 + S2Cl2 1. How many grams of carbon disulfide (CS2) are needed to react with 62.7 g of chlorine? 2. How many grams of carbon tetrachloride (CCl4) can be produced from the 62.7 g of chlorine?
The combustion of propane (C3H8) produces CO2 and H20: C3H8 (g) + 502 (g) – 3C02 (g) + 4H20 (g)The reaction of 2.5 mol of 02 (molar mass: 32:00 g/mol) with 4.6 mol of C3H8 (molar mass: 44.10 g/mol) will produce. mol of H20 (molar mass: 18.01 g/mol). Select one: a.3,68 b.2.76 c.2.0 d.1.5 e.36.02
Copper can have improved wear resistance if alloyed with ceramic alumina, Al2O3. If a copper alloy has 8.4 wt % Al2O3, what is its composition in mol %?

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