"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 1.5 L flask with 0.93 atm of carbon monoxide gas and 3.2 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.62 atm of carbon monoxide gas, 2.89 atm of water vapor and 0.31 atm of hydrogen gas. The engineer then adds another 0.23 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits.

Steam reforming of methane ( CH,) produces "synthesls gas," a mixture of carbon monoxlde gas and hydrogen gas, which Is the starting polnt for many 4 Important industrial chemical syntheses. An Industrial chemist studying this reaction fills a 2.0 L flask with 4.7 atm of methane gas and 2.3 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 4.1 atm. Calculate the pressure equilibrium constant for the steam reforming of methane 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 Accessib M 9 hp Ce

"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 200. mL flask with 3.6 atm of carbon monoxide gas and 2.5 atm of water vapor. When the mixture has come t equilibrium she determines that it contains 2.0 atm of carbon monoxide gas, 0.90 atm of water vapor and 1.6 atm of carbon dioxide. The engineer then adds another 1.2 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

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

At a certain temperature, 0.3011 mol of N₂ and 1.781 mol of H₂ are placed in a 4.00 L container according to the following equation: N₂(g) + 3H2(g) + 2NH3(g) At equilibrium, 0.1401mol of N₂ is present. Calculate the equilibrium constant.

"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 will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200. mL flask with 4.6 atm of ammonia gas, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 4.8 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.

this one is asking for atm

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

At a certain temperature, 0.3811 mol of N₂ and 1.761 mol of H₂ are placed in a 4.50 L container according to the following equation: N₂(g) + 3H₂(g) + 2NH3(g) At equilibrium, 0.1001mol of N2 is present. Calculate the equilibrium constant.