Consider the following equilibrium process at 686°C: CO₂(g) + H₂(g) = CO(g) + H₂O(g) The equilibrium concentrations of the reacting spe- cies are [CO] = 0.050 M, [H₂] = 0.045 M. [CO]= 0.086 M, and [H₂O] = 0.040 M. (a) Calculate K for the reaction at 686°C. (b) If we add CO₂ to increase its concentration to 0.50 mol/L, what will the con- centrations of all the gases be when equilibrium is reestablished?

e File Edit View History Bookmarks Profiles Tab Window Help Watch Gilmore Girls x * Dementia Friend C (2 unread) - dt882 x Lobby | Top Hat A www-awu.aleks.com/alekscgi/x/lsl.exe/1o_u-IgNslkr7j8P3jH-IvdWKW_BBZZI6tTytly4Fcfu6zOtOfE Spotify Web Playe... M common Ethical D.. O CHEMICAL REACTIONS Interconverting number of atoms and mass of compound Calculate the number of carbon atoms in a 150.0 g sample of camphor (C10H0). Be sure your answer has a unit symbol if necessary, and round it to 4 significant digits. x10 Explanation Check MAR 13

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Chrome File Edit View History Bookmarks People Tab Window Help 78% O Thu 10:02 PM A ALEKS - Jacqueline Hoppenrey x A www-awn.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IQİHQRDYV_6Ux63SypJXz0Coxvwqgg4JkWI7XM99oekXTcojkLT31OZqp4772m0XOsdozQ5qMD3aRdEyOGQe33sgOsaJ. O GASES Calculating partial pressure in a gas mixture Jacqueline A 5.00 L tank at 7.37 °C is filled with 18.2 g of chlorine pentafluoride gas and 3.28 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. 圖 mole fraction: chlorine pentafluoride partial pressure: | atm mole fraction: boron trifluoride partial pressure: | atm Total pressure in tank: | atm Explanation Check O2021 McGraw-Hill Education All Rights Reserved Terms of Use Privacy Accessibility MacBook Air 山回

Help 100% 47 T. "ublic Health Ch HSC 258 - Major Projec x MindTap - Cengage Lea X C The Illustration To T =55750828934189288909969212&elSBN=9781305657571&id=D1061392007&nbld=21... * Q Search t Referonces Use the References to access important values if needed for this question. For the following reaction, 50.4 grams of sulfur dioxide are allowed to react with 17.9 grams of water. sulfur dioxide (g) + water (I) sulfurous acid (H2SO3) (g) grams What is the maximum amount of sulfurous acid (H,SO3) that can be formed? What is the FORMULA for the limiting reagent? grams What amount of the excess reagent remains after the reaction is complete? Submit Answer

2.2.1 Gene T x m Inbox (9,414 × M Verify your e X My Question x Things I Can x Course Hom x + USC A openvellum.ecollege.com/course.html?courseld=16196689&HepID=aeb74d6324e98a415a0c4c5c32b9c2e6#10001 I Review | Constants | Periodic Table MISSED THIS? Read Section 16.6 (Pages 696 - 699) ; Watch IWE 16.5 . Part A Consider the following reaction: Fe3+ (aq) + SCN (aq) = FESCN²+ (aq) A solution is made containing an initial Fe+ of 1.2x10-3 M and an initial [SCN ] of 8.1×10-4 M . At equilibrium, [FESCN²+] = 1.8×10-4 M . Calculate the value of the equilibrium constant (Kc). Express your answer using two significant figures. View Available Hint(s) Πνα ΑΣφ ? K = Submit Previous Answers Request Answer * Incorrect; Try Again; 2 attempts remaining Provide Feedback Next :