need help with this chemistry ALEKS - Harrison Felix - Learn X G Calculating an equilibrium consta X +M Gmailwww-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-liGOe3ZhgGhYRBIX9D1jAYn5Rlqv6WMd_eBm5plV8rDcBNiB2WKzMU7cvRstDIP55F3qFVV6qABb8cqJaFZDOQgZKWQAjqq... QCSC-142-Java/my-a... G college proposal un... FCSC143 1VH 21801...YouTube57°FMostly cloudyMapsNew Tab F. HomeHUsed ThankfulGener...You could write down the concentration equilibrium constant expression from the balanced chemical equation -- but you're not given that. You are, however,given a description of the reaction, and you can use that to construct the chemical equation, provided you remember how to go from the names of binarychemicalal compounds to their chemical formulae, and how to balance a chemical equation:4NH₂(g) + 30₂ (g) — 2N₂(g) + 6H₂0 (8)With the chemical equation you can construct the concentration equilibrium constant expression:Nj[HojK= [NH₂] [9₂]The next step is to find the equilibrium molarities to put into this expression, and here there may seem to be a snag: you're only given the equilibrium moles ofthe N₂. What about the rest of the reactants and products?What's important here is not to forget your skills in stoichiometry when you're focused on solving equilibrium problems. Remember that if you know the changein amount of any one reactant or product, you can solve for the change in the amounts of any other reactant or product by using the chemical equation.For example, the rise in moles of H₂O is equal to the rise in moles of N, multiplied by the ratio of their stoichiometric coefficients:6change in H₂O = (change in N₂) = (3.0) = 9.000... molYou can use relationships like this to solve for all the equilibrium moles, and then divide by the volume of the tank to get equilibrium molarities.Another approach is to write an ICE table, even though you're not going to use it to solve a quadratic equation. Let's see what the ICE table for this reactionlooks like when you let stand for the rise in molarity of N.Q Searchinitialchangeequilibrium0.3280-2x0.3280-2xANSWER[NH]= 0.3280-2 (0.02400) = 0.2800.[0₂] = 0.06000-(0.02(0.02400)= 0.02400[N₂] = 0.02400..[H₂0]= 3(0.02400) = 0.07200...(0.02400)²-(0.07200)"(0.2800)*- (0.02400)"X = 9.4 x 10-4[9₂]0.060000.06000*Don't forget to round your final answer to 2 significant digits.What's useful about this ICE table is that you already know X: you're told the equilibrium moles of N₂ is 3.0 mol, and dividing by the volume of the tank givesyou its equilibrium molarity x = 0.02400 mol/L. So if you substitute 0.02400 for x in all the expressions on the "equilibrium" line of the ICE table -- why, thereare your equilibrium molarities, ready to put into the equilibrium constant expression.= 9.444 x 10-4([N] [H₂O00xNow you're ready substitute the equilibrium molarities into the equilibrium constant expression to find :x3x3xRemember you'll need to convertmoles to mol/L by dividing each initialamount by the volume of the tank.Keep a few extra digits for now, and onlyround your final answer to the requestednumber of significant digits.HBMI CalculatorJava Chapter 15 Fla... GSign in - Google Ac...0 XUpdate:11:46 AM5/9/2023 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 a5.0 L flask with 2.0 atm of sulfur dioxide gas and 4.0 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfurtrioxide 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 2significant digits.KP0x10

Answered: Image /qna-images/answer/13941724-811c-4549-a861-a525669e3be9.jpg

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 5.0 L flask with 2.0 atm of sulfur dioxide gas and 4.0 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. X S

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 5.0 L flask with 2.0 atm of sulfur dioxide gas and 4.0 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. X S

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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