9.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 192. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 12.38 g water 3.38 g Use this information to find the molecular formula of X.

9.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 192. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 12.38 g water 3.38 g Use this information to find the molecular formula of X.

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

Similar questions

According to the following reaction, how many grams of mercury will be formed upon the complete reaction of 31.3 grams of mercury(II) oxide? 2HgO(s) → 2Hg(l) + O₂(g) ||| g mercury
Consider the following balanced chemical reaction: CaSO3 + 2HCl → SO2 + H2O + CaCl2 If 750.0 grams of hydrochloric acid reacted with an excess of calcium sulfite, how many grams of sulfur dioxide would form?
Refer to the picture below. If 15.0 g of Mg and 150.0 g of AgNo₃ are allowed to react, find the 1. Mass of Mg(NO₃)₂ that will formed 2. Mass of Ag that will be produced
If 5.3 g of hydrogen gas is reacted with 12.6 g of oxygen gas to produce water, the hydrogen is the A reagent and the oxygen is the A reagent.
A given compound is analyzed and found to contain only C, H and O. When a 35.79 g sample of this compound is completely combusted in the presence of excess oxygen, the reaction yields 49.19 g of carbon dioxide and 13.43 g of water. What is the empirical formula of this compound?
Imagine that you perform a combination reaction between 60.0 g of sodium metal (Na) with 10.0 g of nitrogen gas (N2). Write the balanced chemical equation
Abel reacts copper with silver nitrate and recovers 5.2 g Ag. However, after mass to mass stoichiometry , he discovers that the maximum yield of silver should have been 9.5 g. What is his percent yield?
Consider the copper thermite reaction, a reaction between two solids that can be initiated with strong heating: 3 CuO(s) + 2 Al(s) → 3 Cu(s) + Al2O3(s) 25.0 g of copper(II) oxide are combined with 25.0 g of Al , and the mixture is heated strongly to react. molar masses (g/mol): CuO - 79.55 Al - 26.98 Cu - 63.55 What is the chemical formula or elemental symbol for the limiting reactant? What is the chemical formula or elemental symbol for the excess reactant?
Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes upon contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams upon contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the reaction of an acid on an alkaline earth metal peroxide, such as barium peroxide. BaO2 + HCl ---> H2O2 + BaCl2 What amount of hydrogen peroxide should result when 1.17 g of barium peroxide is treated with 28.0 mL of hydrochloric acid solution containing 0.0288 g of HCl per mL? _____ g H2O2
Consider the following balanced chemical reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g) What is the maximum mass (in grams) of ammonia (NH3) that can be produced from 9.36 g of N2 and 4.92 g of H2?
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: 2C6H5 Cl + C₂2 HOC13 → C14H9 Cl5 + H₂O chlorobenzene chloral DDT In a government lab, 1167 g of chlorobenzene is reacted with 470 g of chloral. a. What mass of DDT is formed, assuming 100% yield? g b. Which reactant is limiting? Which is in excess? is limiting. Mass= is in excess. c. What mass of the excess reactant is left over? g in excess d. If the actual yield of DDT is 285.0 g, what is the percent yield? Percent yield = % Mass=
5.47 g of potassium chlorate is reacted with 1.55 g sulfuric acid to form chloric acid and potassium sulfate. Calculate the amount of excess reactant left over. Atomic Mass: K: 39.098 g/mol Cl: 35.453 g/mol O: 15.999 g/mol H: 1.008 g/mol S: 32.065 g/mol