Calculating an equilibrium constant from a partial equilibrium composition 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 25.0 L tank with 1.6 mol of ammonia gas and 10. mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.32 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K с = ☐ x10 ☑

Calculating an equilibrium constant from a partial equilibrium composition

Steam reforming of methane ( CH, ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 25.0 L tank with 1.5 mol of methane gas and 2.0 mol of water vapor, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 2.7 mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K. = I

If an equilibrium system has a high value (>1) for K, what does this indicate? How will the concentration of reactants compare to the concentration of products? [P] [R]

For which test tube should your value for the equilibrium constant be most reliable? Justify your selection based on your data and your laboratory experience in completing this procedure. Equilibrium Constant, K Test Tube 1 - 75.0 Test Tube 2 - 88.2 Test Tube 3 - 167 Test Tube 4 - 161 Test Tube 5 - -598 Average Kc = -21.4

What does it mean for a chemical reaction to reach equilibrium?         The rates of the forward and reverse reactions are equal. The concentrations of the reactants and products are also equal.         The rates of the forward and reverse reactions are increasing. The concentrations of the reactants and products are equal.         The rates of the forward and reverse reactions are equal. The concentrations of the reactants and products are constant.         The rates of the forward and reverse reactions are increasing. The concentrations of the reactants and products are also increasing.

Calculate the equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture.

Calculating an equilibrium constant from a partial equilibrium.. Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 2.0 L flask with 3.9 atm of sulfur dioxide gas and 0.74 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 1.2 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K, = [ %3D do x10 Ar Eplanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility FEB tv 23 30 MacBook Air DII DD F12 F11 F10 F9 80 888 F8 F7 F5 F6 F4 F3 esc F2 F1 $ % @ 8. 3 4 5 6 2 U

Calculating an equilibrium constant from a partial equilibrium composition 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 2.0 L flask with 1.2 atm of ammonia gas and 3.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.3 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 X ? olo 18 Ar 8.

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N₂(g) + 2 H₂O(g) 2 H₂(g) + 2NO(g) = -9 K₂=3.x 107 He fills a reaction vessel at this temperature with 15. atm of nitrogen gas and 7.8 atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NO, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NO at right. Round your answer to 1 significant digit. O yes O no 0 atm 0 10 X