At 25°C, the equilibrium constant for the reaction N2(g) + O2(g) 2 2 NO(g) is 4.2 x 10-31. Suppose a container is filled with nitrogen (at an initial partial pressure of 0.41 atm), oxygen (at an initial partial pressure of 0.59 atm), and nitrogen oxide (at an initial partial pressure of 0.22 atm). Calculate the tial pressures of all three gases after equilibrium is reached at this temperature. par-

At 25°C, the equilibrium constant for the reaction N2(g) + O2(g) 2 2 NO(g) is 4.2 x 10-31. Suppose a container is filled with nitrogen (at an initial partial pressure of 0.41 atm), oxygen (at an initial partial pressure of 0.59 atm), and nitrogen oxide (at an initial partial pressure of 0.22 atm). Calculate the tial pressures of all three gases after equilibrium is reached at this temperature. par-

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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Consider the following reaction: 2 NO(g) + Br2(g) ⇌ 2 NOBr(g) At a specific temperature, the equilibrium concentrations were determined to be [NO] = 0.067 M, [Br2] = 0.072 M, and [NOBr] = 0.142 M. Based on the value of the equilibrium constant, describe the position of the equilibrium. the position of equilibrium lies to the left, hence the reaction will contain a high concentration of NO and Br2. The position of equilibrium lies to the right, hence the reaction will contain a higher concentration of NOBr. the position of equilibrium lies to the right, hence the reaction will contain a high concentration of NO and Br2. The position of equilibrium lies to the left, hence the reaction will contain a high concentration of NOBr.
At a certain temperature, the equilibrium constant K for the following reaction is 0.0041: NO3(g) + NO(g) = ⇒2 NO₂(g) Use this information to complete the following table. There will be very little NO3 and NO. Suppose a 18. L reaction vessel is filled with 0.61 mol of NO₂. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO₂. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 2 NO2(g) P NO3(9) + NO (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 3 NO3(g) + 3NO(g) 6 NO₂(9) ܢܢ 3 ?
The equilibrium constant, Kp, for the following reaction is 1.04x10-² at 548 K. NH4CI(S) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 6.78 L container at 548 K contains 2.85 mol of NH4Cl(s) and 0.113 mol of NH3(g), the partial pressure of HCI(g) is atm.
At a certain temperature, the equilibrium constant K for the following reaction is 0.54: NO,(g) + NO(g) 2 NO,(g) Use this information to complete the following table. 圖 Suppose a 36. L reaction vessel is filled with 0.97 mol of NO,. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO3 and NO. x10 There will be very little NO2. ? olo Neither of the above is true. Ar What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 1.9 2 NO2(9) NO3(9)+NO(g) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0.29 2 NO3(9)+2NO(9) 4 NO,(9) Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility ........................................... ................ . .......... .........
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 NO(g) + Cl₂(g) 2 NOC1 (g) K₂ = 1. x 10 -6 He fills a reaction vessel at this temperature with 13. atm of nitrogen monoxide gas and 17. atm of chlorine gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NOCI, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NOCI at right. Round your answer to 1 significant digit. O yes O no atm 0 X S BEEN 000 Ar
A student ran the following reaction in the laboratory at 303 K:2NO(g) + Br2(g) 2NOBr(g)When she introduced NO(g) and Br2(g) into a 1.00 L evacuated container, so that the initial partial pressure of NO was 1.15 atm and the initial partial pressure of Br2 was 0.408 atm, she found that the equilibrium partial pressure of Br2 was 0.138 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp =
Consider the following reaction at a certain temperature: 4 Fe(s) + 3 O2(g)→ 2 Fe203(s) An equilibrium mixture contains 1.2 mol Fe, 0.00090 mol O2, and 2.0 mol Fez03 all in a 2.0-L container. Calculate the value of K for this reaction. K =
At a certain temperature, the equilibrium constant K for the following reaction is 0.0096 : N,(8) + O,(g) – 2 NO(g) Use this information to complete the following table. Suppose a 13. L reaction vessel is filled with 0.89 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little N2 and 02. There will be very little NO. ? O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 2 NO(9) N,(9)+0,(9) 1, What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 2 N3(9)+20,(9) 4 NO(9) 1.
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200. mL flask with 1.1 atm of ammonia gas, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 1.2 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. K = 0 P X Ś
A chemical engineer is studying the following reaction: 2 H₂S(g)+30₂(g) → 2 SO₂(g) +2H₂O(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 5.0. The engineer charges ("fills") four reaction vessels with hydrogen sulfide and oxygen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B compound H₂S 0₂ SO2 H₂O H₂S 0₂ SO₂ H₂O H₂S 02 SO₂ H₂O pressure 9.08 atm 1.44 atm 10.07 atm 8.80 atm 8.96 atm 1.26 atm 10.19 atm 8.92 atm 10.40 atm 3.42 atm 8.75 atm 7.48 atm expected change in pressure ↑ increase O decrease ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase O decrease ↑ increase decrease O decrease ↑ increase O decrease ↓ decrease O decrease ↓ decrease O…