The vapor pressure of liquid carbon disulfide, CS2, is 100. mm Hg at 268 K. A 0.261 g sample of liquid CS2 is placed in a closed, evacuated 400. mL container at a temperature of 268 K. Assuming that the temperature remains constant, will all of the liquid evaporate? What will the pressure in the container be when equilibrium is reached? mm Hg

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 2.0 L flask with 3.1 atm of carbon monoxide gas and 3.6 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.0 atm of carbon monoxide gas, 1.5 atm of water vapor and 2.1 atm of carbon dioxide. The engineer then adds another 0.90 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. 0 atm x10 C [

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At a certain temperature, 0.940 mol SO, is placed in a 2.00 L container. 2 SO, (g) = 2 SO,(g) + 0,(g) At equilibrium, 0.130 mol O, is present. Calculate K. K. =

ating UP bunE Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquld form It is easily transported. An Industrial chemist studying this reaction fills a 200. mL flask with 1.6 atm of ammonia gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.7 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = Check Explanation 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibility M 9 hp esc

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 1.5L flask with 2.9 atm of carbon monoxide gas and 2.9 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.4 atm of carbon monoxide gas, 1.4 atm of water vapor and 1.5 atm of carbon dioxide. The engineer then adds another 0.97 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 Submit Assignment Continue 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility MacBook Air DII 888 F10 F8 F9 esc F6 F7 F4 F5 F3 F2 %23 $4 % - & 4. 5 8.

Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 1.5 L flask with 1.7 atm of ammonia gas and 2.1 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 0.77 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = ☐ P x10

Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4(9) +20 2(g) =CO2(g) + 2H 20(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is reduced? O a. The equilibrium position is shifted to the left and the value for K increases. O b. The equilibrium position is shifted to the right and the value for K increases. O c. The equilibrium position is shifted to the right and the value for K decreases. O d. The equilibrium position is shifted but the value for K stays constant. Oe. The equilibrium position is shifted to the left and the value for K decreases.

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g)3H₂(g) + C₂H₂ (g) K₂=6. x 108 He fills a reaction vessel at this temperature with 11. atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of H₂ at right. Round your answer to 1 significant digit. yes no at atm x10 X

Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOX") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 2.0 L flask with 2.9 atm of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 1.4 atm of nitrogen dioxide gas. The engineer then adds another 1.5 atm of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the pressure of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm ☐ x10 X