Suppose a 500. mL flask is filled with 1.4 mol Of OC12, 2.0 mol of BrOCI and 0.60 mol of BrC1. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrC1 (g) The equilibrium constant & for this reaction is 0.371 at the temperature of the flask. Calculate the equilibrium molarity of Broci. Round your answer to two decimal places. Пм

Suppose a 500. mL flask is filled with 1.4 mol Of OC12, 2.0 mol of BrOCI and 0.60 mol of BrC1. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrC1 (g) The equilibrium constant & for this reaction is 0.371 at the temperature of the flask. Calculate the equilibrium molarity of Broci. Round your answer to two decimal places. Пм

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 equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.1 x 103 at a certain temperature. If the equilibrium concentrations of H2 and F2 are both 0.0021 M, determine the concentration of HF at equilibrium. 1 H2(g) +F2(g) 2 HF(g) = 2 NEXT > If [x] represents the equilibrium concentration of HF, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Kc = = 2.1 × 103 RESET [0] [0.0021] 2[0.0021] [x] [2x] [x]2 [2x]2 [0.0011] 2[0.0011] [0.0011]² -Book Air
Suppose a 250. mL flask is filled with 0.60 mol of CHCI,, 0.50 mol of HCl and 1.7 mol of CCI4. The following reaction becomes possible: 3' Cl, (g) + CHCI, (g) – HC1 (g) + CCI4(g) The equilibrium constant K for this reaction is 0.748 at the temperature of the flask. Calculate the equilibrium molarity of CHC1,. Round your answer to two decimal places. M
Suppose a 500. mL flask is filled with 0.60 mol of CO, 0.30 mol of NO and 1.7 mol of CO,. The following reaction becomes possible: NO,(g) +cO(g) - NO(g) +CO, (g) The equilibrium constant K for this reaction is 0.953 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. ?
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Suppose a 250. mL flask is filled with 0.40 mol of OCl,, 1.6 mol of BrOCl and 1.8 mol of BrCl. The following reaction becomes possible: Br, (g) + OCI, (g) - BROCI (g)+ BrCl (g) The equilibrium constant K for this reaction is 0.756 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. OM
Suppose a 500, mL, flask is filled with 1.9 mol of H and 1.6 mol of HI. The following reaction becomes possible: H2(g) + I2(g) ~ 2HI (p) The equilibrium constant K for this reaction is 6.54 at the temperature of the flask. Calculate the equilibrium molarity of I2, Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 1.8 mol of CO, 1.9 mol of H,0 and 1.6 mol of H,. The following reaction becomes possible: co (g) +H,0(g)– CO,(g) +H2 (g) The equilibrium constant K for this reaction is 0.275 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 0.90 mol of Cl₂, 1.2 mol of HCl and 2.0 mol of CC14. The following reaction becomes possible: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) The equilibrium constant K for this reaction is 0.702 at the temperature of the flask. Calculate the equilibrium molarity of CHC13. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 1.7 mol of Br,, 1.4 mol of OCl, and 1.6 mol of BrCl. The following reaction becomes possible: Br, (g) +OCl, (g)- BROC1(g)+BrC1(g) The equilibrium constant K for this reaction is 0.645 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places. olo ? Ar G Explanation Check © 2022 McGraw Hill LLC. AIL Rights Reserved. Terms of Use | Privacy Center | Accessibility
Suppose a 500. mL flask is filled with 1.9 mol of O, and 1.8 mol of SO2. This reaction becomes possible: 2s0,(g) +0,(g) – 2so,(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity. So, O2 initial 口 D. change equilibrium
||| = Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 193.: CO(g) + H₂O(g) - CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 23. L reaction vessel is filled with 1.2 mol of CO₂ and 1.2 mol of H₂. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. CO₂(g)+H₂(g) 2 CO(g) + H₂O(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 CO(g)+2H₂O(g) - 2 CO₂(g) + 2H₂(g) Exmlanation Check Q Search O There will be very little CO and H₂O. O There will be very little CO₂ and H₂. O Neither of the above is true. K = 0 K = 0 X W Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Ce ? S HH