1. Determine the Empirical Formulas from the % Composition data. Compound A: Compound A has a % composition (by mass) of 59.96% C, 26.62% O, and 13.42% H Compound A effuses 1.478 times faster than Xenon gas Compound B: Compound B has a % composition (by mass) of 62.04% C, 27.55% O, and 10.41% H Compound B effuses 1.063 times faster than Xenon gas

1. Determine the Empirical Formulas from the % Composition data. Compound A: Compound A has a % composition (by mass) of 59.96% C, 26.62% O, and 13.42% H Compound A effuses 1.478 times faster than Xenon gas Compound B: Compound B has a % composition (by mass) of 62.04% C, 27.55% O, and 10.41% H Compound B effuses 1.063 times faster than Xenon 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

Chapter5: Gases

Section: Chapter Questions

Problem 147AE: An organic compound contains C, H, N, and O. Combustion of 0.1023 g of the compound in excess oxygen...

See similar textbooks

Similar questions

How would the graph in Figure 9.12 change if the number of moles of gas in the sample used to determine the curve were doubled?
An organic compound contains C, H, N, and O. Combustion of 0.1023 g of the compound in excess oxygen yielded 0.2766 g CO2 and 0.0991 g H2O. A sample of 0.4831 g of the compound was analyzed for nitrogen by the Dumas method (see Exercise 129). At STP, 27.6 mL of dry N2 was obtained. In a third experiment, the density of the compound as a gas was found to be 4.02 g/L at 127C and 256 torr. What are the empirical and molecular formulas of the compound?
A 230-L sample of a colorless gas at STP decomposed to give 230 L of N2 and 1.25 L of O2 at STP. What is the colorless gas?
A hydrocarbon gas has a density of 1.22 g/L at 20C and 1.00 atm. An analysis gives 80.0% C and 20.0% H. What is the molecular formula?
If an electric current is passed through molten sodium chloride, elemental chlorine gas is generated as the sodium chloride is decomposed. :math>2NaCl(1)2Na(s)+Cl2(g) at volume of chlorine gas measured at 767 mm Hg at 25 °C would be generated by complete decomposition of 1.25 g of NaCl?
Explain why the numbers of molecules are not identical in the left- and tight-hand bulbs shown in the center illustration of Figure 9.27.
A Boron and hydrogen form an extensive family of compounds, and the diagram below shows how they are related by reaction. The following table gives the weight percent of boron in each of the compounds. Derive the empirical and molecular formulas of compounds A-E.
Tin(IV) chloride is used as an external coating on glass to toughen glass containers. It is prepared by reacting tin with chlorine gas. Sn(s)+2Cl2(g)SnCl4(l)The process requires a 25.0% excess of tin and has a yield of 73.7%. Calculate the mass of tin and the volume of chlorine gas (d=2.898g/Lat 25C, 1 atm) needed to produce 0.500 L of SnCl4(d=2.226g/mL).
2Fe2O3+3C-4Fe+3CO2The mole ratio for Fe2O3 to CO3 is what in fraction form
Hydrogen gas can be prepared by the reaction of zinc with hydrochloric acidas shown below:2 HCl (aq) + Zn (s) → ZnCl2 (aq) + H2 (g)Calculate the volume of hydrogen gas that is produced at 20.0 C and740. mm Hg from 2.750 g of zinc and an excess of hydrochloric acid
Calculate and show solution 1. Chlorine pentafluoride (CIF₅) is formed by reacting clorine gas (Cl₂) and fluorine gas (F₂). Calculate the volume (in L) of CIF₅ that can be formed from 9.80 L of F₂ at 100°C and a pressure of 1.atm.
Assume that 13.5g of solid aluminum react with excess HCl according to the following balanced equation at 19.0 °Cand 1.12atm: ???(?)+????(??)→??????(??)+???(?) a. How many moles of HCl are used in the reaction? b. What volume of hydrogen gas is produced?