-cnow-owl.cengagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator-assignment-take S ot ts This question has multiple parts. Work all the parts to get the most points. [References] Phosphorus pentachloride decomposes at high temperatures. PCl5 (g) PC13 (g) + Cl2 (g) An equilibrium mixture at some temperature consists of 3.56 g of PCl5, 4.86 g of PCl3, and 3.59 g of Cl2 in a 1.00-L flask. a If you add 1.31 g of Cl2, how will the equilibrium be affected? shift left shift right no shift will occur pt pts 1 pt b What will the concentration of PC15 be when equilibrium is reestablished after addition of 1.31 g Cl₂? 1 pt [PC15] = mol/L 1 pt Submit 1 pt 1 pt Submit Answer Try Another Version 4 item attempts remaining ent 80 a F4 F2 F3 # SA % Cengage Learning | Cengage Technical Support F5 1 MacBook Air F6 A DII F7 F8 * A F9

-cnow-owl.cengagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator-assignment-take S ot ts This question has multiple parts. Work all the parts to get the most points. [References] Phosphorus pentachloride decomposes at high temperatures. PCl5 (g) PC13 (g) + Cl2 (g) An equilibrium mixture at some temperature consists of 3.56 g of PCl5, 4.86 g of PCl3, and 3.59 g of Cl2 in a 1.00-L flask. a If you add 1.31 g of Cl2, how will the equilibrium be affected? shift left shift right no shift will occur pt pts 1 pt b What will the concentration of PC15 be when equilibrium is reestablished after addition of 1.31 g Cl₂? 1 pt [PC15] = mol/L 1 pt Submit 1 pt 1 pt Submit Answer Try Another Version 4 item attempts remaining ent 80 a F4 F2 F3 # SA % Cengage Learning | Cengage Technical Support F5 1 MacBook Air F6 A DII F7 F8 * A F9

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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Hydrogen chloride decomposes to form hydrogen and chlorine, like this: 2 HCl(g) - H2(9) + Cl,(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following composition: compound concentration at equilibrium HC1 0.49 M H, 1.9M Cl, 0.10M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K̟ = 0
Identify the proper form of the equilibrium-constant expression for the equation N2 (g) + O2 (g) = 2NO(g) • View Available Hint(s) [NO] Ο Κ: [N2][O2] [NO]? O K: [N2][O2] 12 [N2][O2] O K = [NO]? 2[NO] Ο Κ- [N2][O2]
Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N204(g) = 2 NO2(2) Three experiments were run starting with different initial amounts of N2O4(g) ([N2O4lo in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO, and N,04 at equilibrium. Be sure to round to the correct number of significant figures. Exp N,04lo NO,] N,04] NO,] / [N,04 2 [NO,] / [N,04 NO,1? / [N,04] 1 3.7 2.92 2.2 2 3.0 2.56 1.7 3 2.3 2.15 1.2 Based on your calculations, indicate whether each statement is True (T) or False (F): v1. Each experiment started with a different initial concentration of N,O4. v 2. The ratio ([NO,] / [N,O4]) is equal to a constant value. 3. The ratio (2 [NO,] /…
Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s)+3 H,0(g)→ Fe,O3(s)+3 H,(g) At a certain temperature, a chemist finds that a 9.2 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound amount ol. Fe 4.85 g Ar H,O 1.44 g Fe,O3 2.98 g H2 2.51 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 Ox10 Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
9 q eq eq req req 1req OWLv2 | Online teaching and learning resource from Cengage Le... Submit Answer [Review Topics] [References] Use the References to access important values if needed for this question. The equilibrium constant, Kp, for the following reaction is 0.497 at 500. K. PC15 (9) PC13 (g) + Cl₂ (g) If an equilibrium mixture of the three gases in a 12.7 L container at 500. K contains PC15 at a pressure of 0.804 atm and PC13 at a pressure of 0.911 atm, the equilibrium partial pressure of Cl₂ is l atm. b Home | bartleby Retry Entire Group 9 more group attempts remaining
3.) For the following equilibrium reaction2NO2(g) ↔N2O4(g) + Δlook in the Tro text to see what LeChatelier's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. [Hint: remember that PV=nRT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.
[References] The equilibrium constant for the reaction PCl, 2 PC13 + Cl2 is 0.0245 at 250.°C. What molar concentration of PCl; would be present at equilibrium if the concentrations of PCI3 and Cl2 were both 0.161 M? Molar concentration of PCI3 = M
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 302(g)=20, (g) K = 1.x 10-2 He fills a reaction vessel at this temperature with 9.0 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 yes available to you within ALEKS? If you said yes, then enter the equilibrium pressure of O, at right. Round your answer to 1 significant digit. O no X Oatm
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 302(g)=203(g) -2 Kp =4. x 10 He fills a reaction vessel at this temperature with 15, 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? If you said yes, then enter the equilibrium pressure of 03 at right. Round your answer to 1 significant digit. yes ☐ x10 O no X ☐ atm
In air at 25 °C and 1.00 atm, the N₂ concentration is is 0.033 M. The 0.01 M and the O₂ concentration reaction N₂(g) + O₂(g) → 2NO(g) has Kc = 4.8 x 10-31 at 25 °C. C Taking the N₂ and O2 concentrations given above as initial values, calculate the equilibrium NO concentration that should exist in our atmosphere from this reaction at 32 °C, Kc = 2.6E-30. Make simplifying assumptions in your calculations. (Express your answer in scientific notation.) [NO] = i M !
Suppose a 500. ml flask is filled with 0.50 mol of SO, and 0.30 mol of SO,. This reaction becomes possible: 2s0,(e) +0,(x) - • 250, (e) Complete the table below, so that it lists the initial molarity of cach 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, so, Initial change equilibrium
for equilibrium 2SO2 + O2 = 2SO3, the initial concentrations are [SO2] = 0.9 and [O2] = 0.8. At the moment of equilibrium [SO3] = 0.4. The value of the equilibrium constant is: a) 0.08 b) 1.06 c) 0.16 d) 1.08