CHEMWORKThe reaction H,(g) + I(g) 2 2HI(g) has K, = 45.9 at 763 K. A particular equilibrium mixture at 763 K contains HI at a pressure of 3.28 atm and H, at a pressure of 1.20 atm. Calculate the equilibrium pressure of I,(g) in this mixture.atmPLSubmitSubmit AnswerTry Another Version1 item attempt remaining(Previousywww.yahoo.com 2h ATop StoryNew research raises doubts about 1 stCOVID-19 death countCengage Learning | Cengage Technical SupportDELL

Answered: Image /qna-images/answer/66d7c87c-36ca-41de-8e70-b97a07bd8192.jpg

CHEMWORK The reaction H(g) - 1(g) = 2HI(g) has K. = 45.9 at 763 K. A particular equilibrIum mixture at 763 K contains HI at a pressure of 3.28 atm and H2 at a pressure of 1.20 atm. Calculate the equilibrium pressure of L(g) in this mixture. atm Submit Submit Answer Try Another Version 1 item attempt remaining

CHEMWORK The reaction H(g) - 1(g) = 2HI(g) has K. = 45.9 at 763 K. A particular equilibrIum mixture at 763 K contains HI at a pressure of 3.28 atm and H2 at a pressure of 1.20 atm. Calculate the equilibrium pressure of L(g) in this mixture. atm Submit Submit Answer Try Another Version 1 item attempt 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...

See similar textbooks

Similar questions

okmarks People Tab Window Help Chem101 Question 2 of 9 Consider the reaction: 2 A (g) + B (s) = 2 C (s) + D (g) To increase the partial pressure of D at equilibrium, you could
Q Search this course Reference Use the References to access importantv needed for this question. The equilibrium constant, K, for the following reaction is 1.20x102 at 500 K PCI5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.164 M PCI 4.43x10 M PCI3 and 4.43x10 M C2. What will be the concentrations of the three gases equilibrium has been reestablished, if 2.27x10 mol of Ch(g) is added to the flask? once [PCI5]= [PCI3]= М [Cl2] sturbing Equilibrium Concentrations (Qua... : This is group attempt 1 of 5 Next ack 1:33 PM 9/24/2019 up Xx
How can we solve this?
um problems A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 302(g)=203(g) K=2. × 10 P He fills a reaction vessel at this temperature with 14. atm of oxygen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of O3, using only the tools available to you within ALEKS? yes x10 по If you said yes, then enter the equilibrium pressure of 03 at right. Round your answer to 1 significant digit. X- atm
I need full details answer and accurate answer please.
These are practice questions. Please help! Thanks.
Dear expert don't use Ai plz 2 downvotes
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 5.0 L 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 0.50 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. dlo K -1 Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility 23 MacBook Alr
At 1100 K, Kp = 0.32 for the reaction 2SO₂(g) + O₂(g) ⇒ 2SO3 (9) What is the value of K at this temperature? K= Submit Answer Try Another Version 1 item attempt remaining
At 25°C, gaseous SO2 Cl2 decomposes to SO2 (9) and Cl2 (g) to the extent that 13.8% of the original SO, Cl, (by moles) has decomposed to reach equilibrium. The total pressure (at equilibrium) is 0.740 atm. Calculate the value of K, for this system. K, = Submit Answer Try Another Version 5 item attempts remaining
Question 2 of 7 Submit You re studying the reaction A2 (g) + 3 B2 g) = 2 AB3 (g) and you find that Kp for this reaction is 11.2. At equilibrium, you find the partial pressure of A2 = 0.125 atm and the partial pressure of B2 = 0.250 atm. What is the equilibrium pressure of AB3? 1 2 3 4 6. C 7 8 +/- х 100 Tap here or pull up for additional resources LO
" 2 H₂S(g) 2 H₂(g) + S₂(g) Kc = 9.3x 108 at 400°C 0.25 moles of H₂S are placed in a 3.0 L container and the system is allowed to reach equilibrium. Calculate the concentration of H₂ at equilibrium. 2.0 × 10-3 M 1.1 x 10-3 M (Correct answer) 5.4 x 104 M 8.8 × 10-5 M 1.9 × 10-9 M