Use the References to access important values if needed for this question. he equilibrium constant, K, for the following reaction is 2.20x101 at 723K. 2NH3(g) N2(g) + 3H2(g) If an equilibrium mixture of the three gases in a 11.8 L container at 723K contains NHa at a pressure of 0.588 atm and N, at a pressure of 0.774 atm, the equilibriL pressure of H2 is atm. Submit Answer Try Another Version 3 item attempts remaining

Use the References to access important values if needed for this question. he equilibrium constant, K, for the following reaction is 2.20x101 at 723K. 2NH3(g) N2(g) + 3H2(g) If an equilibrium mixture of the three gases in a 11.8 L container at 723K contains NHa at a pressure of 0.588 atm and N, at a pressure of 0.774 atm, the equilibriL pressure of H2 is atm. Submit Answer Try Another Version 3 item attempts remaining

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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.
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 N,(g) + 3 H,(g) 2 NH3(g) K = 1. × 10 He fills a reaction vessel at this temperature with 10. atm of nitrogen gas and 3.9 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes tools available to you within ALEKS? no ? If you said yes, then enter the equilibrium pressure of NH, at right. atm Round your answer to 1 significant digit.
"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.
Consider the following reaction. 2 NO, (g) = N,04(g) When the system is at equilibrium, it contains NO, at a pressure of 0.872 atm, and N,O, at a pressure of 0.0760 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? PNO, = atm PN,0, atm
The equilibrium constant, K,, for the following reaction is 2.74 at 1.15x1o3K. 2503(g) 2s02(g) + 02(g) If an equilibrium mixture of the three gases in a 16.5 L container at 1.15×103K contains soz at a pressure of 1.62 atm and So, at a pressure of 1.04 atm, the equilibrium partial pressure of O, is atm.
Suppose a 250. mL flask is filled with 0.30 mol of NO and 0.80 mol of NO2. The following reaction becomes possible: NO3(g)+NO(g)<->2NO2(g) The equilibrium constant K for this reaction is 0.717 at the temperature of the flask. Calculate the equilibrium molarity of NO2. Round your answer to two decimal places.
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant k for the following reaction is 9.84 x 101: N,(g) + 0,(g) = 2 NO(g) Use this information to complete the following table. Suppose a 30. L reaction vessel is filled with 0.64 mol of N2 and There will be very little N, and O2. alo 0.64 mol of 0,. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K 2 NO(g) N3(9)+Og(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = 3 N,(9)+30,(9) 6 NO(g)
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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
Use the References to access important values if needed for this question. The equilibrium constant, K for the following reaction is 6.50×10 at 298K. 2NOBR(g)=2NO(g) + Br,(g) If an equilibrium mixture of the three gases in a 17.2 L container at 29SK contains 0.369 mol of NOBR(g) and 0.435 mol of NO, the equilibrium concentration of Br, is M.
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.
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.