Phosphorus tribromide decomposes to form phosphorus and bromine, like this: 4 PB13(g) → P4(g) + 6 Br,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of phosphorus tribromide, phosphorus, and bromine has the following composition: compound concentration at equilibrium 0.66M P4 0.79M Br, 0.62M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K =

Phosphorus tribromide decomposes to form phosphorus and bromine, like this: 4 PB13(g) → P4(g) + 6 Br,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of phosphorus tribromide, phosphorus, and bromine has the following composition: compound concentration at equilibrium 0.66M P4 0.79M Br, 0.62M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K =

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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Hydrogen chloride decomposes to form hydrogen and chlorine, like this: 2 HCl(g) H,(g) + Cl,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following composition: compound concentration at equilibrium HC1 0.73 М H2 1.2M Cl2 0.90M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = [] %3D 10 Explanation Check O 2022 McGraw Hill LLC. AlI Rights Reserved. Terms of Use Privacy Center Access DELL Esc F1 F2 F3 F4 F5 U F6 F7 F8 F9 F10 F11 F12 PrtScr Insert Delete "R # $ & Num Lock 1 2 3 4 Backspace 7 Tab R Y * 00
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Using the general properties of equilibrium constants 0/5 At a certain temperature, the equilibrium constant K for the following reaction is 7.4 × 10 ': N,(e) + 0,(g) -2NO(g) Use this information to complete the following table. Suppose a 35. L reaction vessel is filled with 1.7 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little N, and 0,. O 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 =] 2 NO(g) N2(0)+O2(a) 1, What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] 2N,(0)+20,(0) 4 NO(g) 1,
Hydrogen chloride decomposes to form hydrogen and chlorine, like this: 2 HCl(g) - H2(9) + Cl,(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following composition: compound concentration at equilibrium HC1 0.49 M H, 1.9M Cl, 0.10M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K̟ = 0
A chemical engineer is studying the following reaction: 2 NO(g)+2H,(9) - N2(9)+2H,0(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 2.0. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, 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 compound pressure expected change in pressure vessel ΝΟ 6.78 atm O f increase Ot decrease O (no change) H, 2.93 atm ↑ increase OI decrease O (no change) A N2 5.23 atm f increase I decrease (no change) H, O 7.24 atm t increase I decrease (no change) NO 5.29 atm f increase I decrease (no change) H, 1.44 atm f increase OI decrease (no change) В N2 5.98 atm increase I decrease (no change) H, O 8.73 atm f increase O I decrease O (no change)…
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.
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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) К, — 3. х 10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 3.2 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 x10 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.