Suppose a 250. mL flask is filled with 0.20 mol of Cl\(_2\), 1.0 mol of CHCl\(_3\), and 2.0 mol of CCl\(_4\). The following reaction becomes possible:\[ \text{Cl}_2(g) + \text{CHCl}_3(g) \rightleftharpoons \text{HCl}(g) + \text{CCl}_4(g) \]The equilibrium constant \( K \) for this reaction is 8.66 at the temperature of the flask.Calculate the equilibrium molarity of Cl\(_2\). Round your answer to two decimal places.

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Answered: Suppose a 250. mL flask is filled with…

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

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Suppose a 250. mL flask is filled with 1.8 mol of CO, 0.20 mol of H2O and 1.0 mol of H2. The following reaction becomes possible: CO(g)+H,O()-CO,(z)+H.() The equilibrium constant K for this reaction is 2.64 at the temperature of the flask. Calculate the equilibrium molarity of H2O. Round your answer to two decimal places. Ом 5
Suppose a 250. mL flask is filled with 1.9 mol of Br,, 1.8 mol of BrOCl and 1.6 mol of BrCl. The following reaction becomes possible: Br, (g) + OC1, (g) = BIOC1(g) + BrC1(g) The equilibrium constant K for this reaction is 4.15 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. 0.53 M ?
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Suppose a 500. mL flask is filled with 1.9 mol of H, and 1.1 mol of NH,. This reaction becomes possible: N, (g) +3H,(g) =2NH, (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 N,. You can leave out the M symbol for molarity. olo Ar N2 H, NH, initial change equilibrium 미
Suppose a 250. mL flask is filled with 1.6 mol of CH, 1.8 mol of H,O and 0.70 mol of CO. This reaction becomes possible: () +H,0(g) C0(g) +3H,(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 CO. You can leave out the M symbol for molarity. CH, H,0 CO H, initial change equilibrium Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use| Privacy I Accessibility 口ロ X
Suppose a 500. mL flask is filled with 1.7 mol of OCl2, 0.70 mol of BrOCI and 1.1 mol of BrCl. The following reaction becomes possible: Br2(g) +OCl2(g) BrOCI(g) + BrCl (g) The equilibrium constant K for this reaction is 3.84 at the temperature of the flask. Calculate the equilibrium molarity of OCl2. Round your answer to two decimal places. ☐ M ☑
At a certain temperature, 0.960 mol SO, is placed in a 2.50 L container. 2 SO, (g) = 2 SO,(g) + 0,(g) At equilibrium, 0.190 mol O, is present. Calculate K. K. =
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI,(g) + Cl, (g) Ke = 1.80 at 250 °C A 0.1978 mol sample of PCl, (g) is injected into an empty 3.15 L reaction vessel held at 250 °C. Calculate the concentrations of PCI, (g) and PCI, (g) at equilibrium. [PCI,] = %3D [PCI,] = M %3D Question Source: MRG - General Chemistry | Pul terms of use | help about us careers privacy policy contact us N prime video P II
At 400 K, an equilibrium mixture of H2, 12, and HI consists of 0.065 mol H2, 0.079 mol 12, and 0.13 mol HI in a 4.50-L flask. What is the value of K, for the following equilibrium? (R= 0.0821 L atm/(K • mol)) 2HI(g) = H2(g) + 12(8) 0.29 8.2 0.039 O 26 3.4
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