Constants | Periodic TablewaiConsider the endothermic decomposition reaction ofchlorine monofluoride at 1107.6 K.SubmitRequest Answer2 CIF(g) = Cl2(g) + F2(g)Part BThe equilibrium constant at 1107.6 K is K = 5.68×10-6.If you were a chemist and trying to maximize the amount of decomposition of CIF, which of the following tactics might you try? Assumethat the mixture reaches equilibrium.Check all that apply.remove F, from the reaction mixture as it forms.O increase the volume of the reaction containerO add a catalyst to increase the rate of decompositionO increase the reaction temperature

In this reaction 2 moles of ClF is decomposing into one mole of Cl2 and one mole of F2. In an…

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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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A 2.20 mole quantity of NOCl was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 32.0 percent of the NOCl had dissociated: 2NOCl(g) 2NO(g) + Cl2(g) Calculate the equilibrium constant Kc for the reaction.
The equilibrium constant for the decomposition of COCl2 to form CO and Cl2 at 900ºC is 8.3 x 10-2.COCl2(g) CO(g) + Cl2(g) K= 8.3 x 10-2 What is the equilibrium constant for the following reaction under the same conditions?3CO(g) + 3Cl2(g)3COCl2(g) K= ? Question 6 options: A) 2.3 B) 1.7 x 103 C) 1.2 x 101 D) 5.7 x 10-4 E) -5.7 x 10-4
The following reaction is exothermic. 2 NO(g) + 2 H2(g) ⇔ N2(g) + 2 H2O(g) In which direction does the equilibrium shift as a result of each of the following changes? Here are the possible answers: to the right, to the left, no effect Place these actions in chronological order. Space 1: The hydrogen gas is removed. Space 2: The gas pressure in the reaction vessel is increased by decreasing its volume. Space 3: The gas pressure in the reaction vessel is increased by pumping argon gas into it while keeping the volume constant. Space 4: We raise the temperature. Space 5: A catalyst is used.
A student ran the following reaction in the laboratory at 695 K:N2(g) + 3H2(g) 2NH3(g)When she introduced 4.09×10-2 moles of N2(g) and 7.14×10-2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 1.99×10-3 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.
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Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)→2 HgO(s) At a certain temperature, a chemist finds that a 7.0 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 7.0 g O2 5.8 g HgO 16.5 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = | x10
The following reaction has an equilibrium constant of 2.65 x10-3 at 300K. Br2 (g) + Cl2 (g) 2 BrCl (g) Which of the following statements is true? Question 5 options: The system has a higher concentration of reactant molecules than product molecules at equilibrium, but there are significant quantities of both. The system consists almost entirely of reactant molecules at equilibrium. The system consists almost entirely of product molecules at equilibrium. The system has approximately equal concentrations of product and reactant molecules at equilibrium. The system has higher concentrations of product molecules than reactant molecules at equilibrium, but there are significant quantities of both.
A chemical engineer is studying the following reaction: H2(9)+Cl2(g) → 2 HCl(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.1. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, and lets the reaction begin. He then measures the 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 pressure expected change in pressure H, 2.75 atm t increase I decrease (no change) Cl, 4.00 atm t increase O I decrease O (no change) A HCI 2.10 atm O f increase OI decrease O (no change) H, 2.78 atm t increase I decrease O (no change) Cl, 4.03 atm t increase I decrease (no change) 2.06 atm t increase I decrease (no change) HCl H2 3.22 atm O f increase I decrease (no change) t increase I decrease (no change) Cl, 4.98 atm OI decrease O (no change) H CI 4.26 atm…
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…
7. Suppose for a synthesis of hydrogen fluoride from hydrogen and fluorine, 3.000 moles of H2 and 6.000 moles of F2 are mixed in a 3.000-L flask. Assume that the equilibrium constant for the synthesis reaction at this temperature is 1.15x102. H2 (g) + F2 (g) ↔ 2HF (g) What is the molar concentration of HF at equilibrium? What is the molar concentration of F2 at equilibrium? At a Kc of 4.15x103, predict the direction of the reaction if the starting concentrations are [H2]=2.30 M, [F2]= 1.25x10-3 M, and [HF]= 4.37 M

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