Consider the synthesis of hydrogen iodide from molecular hydrogen and iodide. At equilibrium a vessel contains a mixture of I2 (purple), H₂ (Colorles) and HI (colorless). The value of Kc=56 at 200k. H₂(g) + Izeg) HI(g) e) IH now ( a) If the purple color of the mixture fades as the temperature is raised is the reaction forming FI exothermic or endothermic? llow sI to tomo 23 19225v silt to Jou N AW CE b) A flask is immersed in a constant-temp. bath maintained @ 200 kelvin. The flask initially contains: [H₂] = 0,024M, [1₂]=0.036 M [HI] = 0.15M. Will the [HI] increase or Stolyola) (s decrease? C) What is the value of Ke for this ran. HI(g) = 1/2 H₂(g) + 1½/2I2(9) Mod 1010 N

Consider the synthesis of hydrogen iodide from molecular hydrogen and iodide. At equilibrium a vessel contains a mixture of I2 (purple), H₂ (Colorles) and HI (colorless). The value of Kc=56 at 200k. H₂(g) + Izeg) HI(g) e) IH now ( a) If the purple color of the mixture fades as the temperature is raised is the reaction forming FI exothermic or endothermic? llow sI to tomo 23 19225v silt to Jou N AW CE b) A flask is immersed in a constant-temp. bath maintained @ 200 kelvin. The flask initially contains: [H₂] = 0,024M, [1₂]=0.036 M [HI] = 0.15M. Will the [HI] increase or Stolyola) (s decrease? C) What is the value of Ke for this ran. HI(g) = 1/2 H₂(g) + 1½/2I2(9) Mod 1010 N

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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At a given temperature, the equilibrium constant (K,) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.188. If 0.295 atm N204 is sealed in a flask, what partial pressure (in atm) of NO2 will exist at equilibrium? N2O4(g) 2 2NO2(3) Type your answer... Submit
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 3.0 L reaction vessel contained a mixture of 1.37 x 10-2 M HI, 6.47 × 10-3 M H2, and 5.94 × 10-4 M I, at 740 K. What are the values of Kc and Kp for the reaction at this temperature? H2(g) + 12(g) = 2 HI(g) 1 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms. K. = 2 RESET [1.37 x 10-2] [6.47 x 10-3] [5.94 × 10-4] [4.57 × 10-3] [2.16 х 10-3] [2.31 x 10-4] 2[1.37 x 10-2] 2[6.47 x 10-3] 2[5.94 x 10-4] [1.37 х 10-7)2 [6.47 x 10-312 [5.94 x 10-4]2 3.56 x 103 2.81 × 10-4 48.8 2.05 x 10-2
A chem gineer is studying the following reaclon! HCN(aq)+NH,(aq) - CN (aq)+NH,(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.99. The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel compound concentration expected change in concentration HCN 0.84 M O t increase OI decrease O (no change) NH, 1.00 M O t increase O, decrease O (no change) CN 0.42 M O 1 increase O. decrease O (no change) NH, 0.33 M O t increase O, decrease O (no change) HCN 1.01 M O t increase O. decrease O (no change) NH, 1.17 M O t increase O. decrease O (no change) CN 0.25 NM M t increase O. decrease O (no change) NH. 0.16 MM O t increase O.…
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.
Iron and water react to form iron (III) oxide and hydrogen, like this: 2 Fe(s)+3 H₂O(g)→Fe₂O3(s)+ 3 H₂(9) At a certain temperature, a chemist finds that a 8.1 L reaction vessel containing a mixture of iron, water, iron (III) oxide, and hydrogen at equilibrium has the following composition: compound amount Fe 1.92 g H₂O 1.12 g Fe₂03 2.32 g H₂ 2.30 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 X
18)The equilibrium constant at 1127 °C for the following endothermic reaction is 571: 2 H₂S (g) 2 H₂ (g) + S₂ (g) If the mixture is at equilibrium, what happens if we a) Add some H₂S b) Add some H₂ c) Lower the temperature to 1000 °C
At a certain temperature, the equilibrium constant K for the following reaction is 0.0096 : N,(8) + O,(g) – 2 NO(g) Use this information to complete the following table. Suppose a 13. L reaction vessel is filled with 0.89 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little N2 and 02. There will be very little NO. ? O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 2 NO(9) N,(9)+0,(9) 1, What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 2 N3(9)+20,(9) 4 NO(9) 1.
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For the reaction 3 O2(g) 2 O3(g) The equilibrium constant, K, has the value 1.12 10-54 at a particular temperature. (b) If the equilibrium mixture is analyzed and [O2(g)] is found to be 3.71 10-2 M, what is the concentration of O3(g) in the mixture? M
Consider the reaction shown below at room temperature. 2H2(g) + S2(g) ⇋ 2H2S(g) The equilibrium constant, K, is equal to 1.1 x 107. A mixture of reactants and products at room temperature contains 0.25 M H2, 0.15 M S2, and 0.50 M H2S. (a) Is this reaction at equilibrium? (b) In which direction does the reaction proceed to reach equilibrium? (c) Assuming the reactants remain at the same equilibrium concentrations, what would the concentration of the product have to be in order to establish equilibrium?
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A chem ngineer is studying the following reaction: + HCN(aq) + NH3(aq) → CN¯(aq)+NH (aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.1. C The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B C compound HCN NH3 CN NH4 HCN NH3 CN NH₁ HCN NH₂ CN NHA 4 concentration 0.28 M 0.12 M 1.05 M 0.94 M 0.67 M 0.51 M 0.66 M 0.55 M 0.31 M 0.15 M 1.02 M 0.91 M expected change in concentration ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↓ decrease ↓decrease ↓ decrease 888888 ↓decrease ↓ decrease ↓decrease ↓ decrease ↓ decrease ↓decrease…