Dimethyl ether, CH3OCH3, undergoes gas phase decomposition to form methane, hydrogen gas, and carbon monoxide. Calculate the total volume of gas products if 66.92 g of dimethyl ether decomposes at 53.44°C and 0.32 atm and the gas completely decomposes. Atomic Mass: C: 12.011 g/mol H: 1.008 g/mol O: 15.999 g/mol Show your solutions in the next item

Dimethyl ether, CH3OCH3, undergoes gas phase decomposition to form methane, hydrogen gas, and carbon monoxide. Calculate the total volume of gas products if 66.92 g of dimethyl ether decomposes at 53.44°C and 0.32 atm and the gas completely decomposes. Atomic Mass: C: 12.011 g/mol H: 1.008 g/mol O: 15.999 g/mol Show your solutions in the next item

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 77E: A 15.0-L rigid container was charged with 0.500 atm of krypton gas and 1.50 atm of chlorine gas at...

See similar textbooks

Similar questions

Given that 1.00 mol of neon and 1.00 mol of hydrogen chloride gas are in separate containers at the same temperature and pressure, calculate each of the following ratios. (a) volume Ne/volume HCI (b) density Ne/density HCI (c) average translational energy Ne/average translational energy HCI (d) number of Ne atoms/number of HCl molecules
A mixture of chromium and zinc weighing 0.362 g was reacted with an excess of hydrochloric acid. After all the metals in the mixture reacted, 225 mL dry of hydrogen gas was collected at 27C and 750. torr. Determine the mass percent of Zn in the metal sample. [Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas; chromium reacts with hydrochloric acid to produce chromium(III) chloride and hydrogen gas.]
Ethanol, C2H5OH, is produced industrially from ethylene, C2H4, by the following sequence of reactions: 3C2H4+2H2SO4C2H5HSO4+( C 2 H 5)2SO4C2H5HSO4+( C 2 H 5)2SO4+3H2O3C2H5OH+2H2SO4 What volume of ethylene at STP is required to produce 1.000 metric ton (1000 kg) of ethanol if the overall yield of ethanol is 90.1%?
Workers at a research station in the Antarctic collected a sample of air to test for airborne pollutants. They collected the sample in a 1.00-L container at 764 torr and 20 C. Calculate the pressure in the container when it was opened for analysis in a particulate-free clean room in a laboratory in South Carolina, at a temperature of 22 C.
The oxides of Group 2A metals (symbolized by M here) react with carbon dioxide according to the following reaction: MO(s)+CO2(g)MCO3(s) A 2.85-g sample containing only MgO and CuO is placed in a 3.00-L container. The container is filled with CO2 to a pressure of 740. torr at 20.C. After the reaction has gone to completion, the pressure inside the flask is 390. torr at 20.C. What is the mass percent of MgO in the mixture? Assume that only the MgO reacts with CO2.
A 15.0-L rigid container was charged with 0.500 atm of krypton gas and 1.50 atm of chlorine gas at 350.C. The krypton and chlorine react to form krypton tetrachloride. What mass of krypton tetrachloride can be produced assuming 100% yield?
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)