Fluoride anion and hydronium cation react to form hydrofluoric acid and water, like this: F (aq)+H₂O (aq)-HF(aq)+H₂O(1) At a certain temperature, a chemist finds that a 5.9 L reaction vessel containing an aqueous solution of fluoride anion, hydronium cation, hydrofluoric acid, and water at equilibrium has the following composition: compound amount F 0.138 g H₂O* 0.217 g HF 1.93 g H₂O 599. g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. S

Fluoride anion and hydronium cation react to form hydrofluoric acid and water, like this: F (aq)+H₂O (aq)-HF(aq)+H₂O(1) At a certain temperature, a chemist finds that a 5.9 L reaction vessel containing an aqueous solution of fluoride anion, hydronium cation, hydrofluoric acid, and water at equilibrium has the following composition: compound amount F 0.138 g H₂O* 0.217 g HF 1.93 g H₂O 599. g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. S

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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1.3 3 (i) In the Haber process for the production of ammonia, the following reaction occurs: 3H2(g) 2NH3(g) AH is negative N2 (g) + If the equilibrium concentrations for all the reactants and products at 600°C are: [N₂] = 0.40 mol/dm³, [H₂] = 1.20 mol/dm³ and [NH3] = 0.20 mol/dm³ Construct an expression for Kc and calculate the numerical value of the equilibrium constant, Kc. (ii) At 500°C Kc 0.062 mol-2dm. Compare this value to the one you calculated in 3(i) above and state whether the yield of ammonia is greater at 500°C or 600°C and briefly explain your choice. =
A mixture of 30.0 mol of NO(g) and 18.0 mol of O2(g) is placed in an empty 3.00-liter flask held at a constant temperature. These gases react until the reaction represented below comes to equilibrium. At equilibrium, the vessel contains 26.4 moles of NO2. What is the value of the equilibrium constant at the constant temperature? 2NO(g) + O2(g)  2NO2(g)
Consider the following system at equilibrium where AH° PC15 (9) PCl3 (g) + Cl₂ (g) O increases decreases O remains the same = If the temperature on the equilibrium system is suddenly increased: The value of K 87.9 kJ, and Ke 1.20 × 10-2, at 500 K: The concentration of Cl₂ will O increase decrease O remain the same The value of Q O is less than Kc O is greater than Kc O is equal to Kc The reaction must O run in the forward direction to reestablish equilibrium O run in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium = Consider the wings All-179 The value of
Iron(III) oxide and hydrogen react to form iron and water, like this: Fe,0;(s)+3 H,(g)→2FE(s)+3H,O(9) At a certain temperature, a chemist finds that a 5.1 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount db Fe,O3 4.36 g H, 4.35 g Fe 3.23 g H,0 2.73 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. Explanation Check 2022 McGraw H LLC. A Rights Reserved Terms of Use Pvacy Center Accessibil DE P Type here to search JU P. Alt alexa ENADLED
The reaction N2(g) + 3 H2(g) ⇀↽ 2 NH3(g), has an equilibrium constant of 4.0 × 108 at 25◦C. What will eventually happen if 44.0 moles of NH3, 0.452 moles of N2, and 0.108 moles of H2 are put in a 10.0 liter container at 25◦C? More N2 and H2 will be formed. Nothing; the system is at equilibrium. More NH3 will be formed.
A chemical engineer is studying the following reaction: HCH3CO2(aq)+CH3NH2(aq) → CH3CO2(aq)+CH3NH(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.80. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound concentration expected change in concentration HCH CO₂ 0.58 M ↑ increase ↓ decrease (no change) CH3NH2 0.57 M ↑ increase ↓ decrease (no change) A CH3CO2 1.09 M ○ ↑ increase ↓ decrease (no change) CH,NH, 1.28 M ○ ↑ increase ↓ decrease (no change) HCH,CO₂ CH3NH2 1.28 M ↑ increase ↓decrease (no change) 1.27 M ↑ increase ↓ decrease (no change) B CH,CO, 0.39 M ↑ increase ↓ decrease (no change) CHÍNH, HCH3CO2…
A chemical engineer is studying the following reaction: + CH3CH,NH,(aq)+HCl(aq) Ci (aq)+CH ,CH,NH,(aq) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.2. The engineer charges ("fills") four reaction vessels with ethylamine and hydrogen chloride, 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 CH,CH,NH, 0.76 M f increase I decrease (no change) H Cl 0.92 M f increase I decrease (no change) A Cl 0.97 M f increase I decrease (no change) CH;CH,NH, 0.88 M f increase I decrease (no change) CH;CH,NH, 0.38 M f increase I decrease (no change) H Cl 0.54 M f increase I decrease (no change) B Cl 1.35 M f increase I decrease (no change) CH,CH,NH, 1.26 M f…
2. Ozone can be created from oxygen gas (with an input of energy) via the following reaction: 30₂(8) = 203 (8) -2 If the equilibrium constant, K, is 1.02 x 10-24 for this reaction at a particular temperature and [0₂] = 3.10 x 10 M at equilibrium, what is [03] (in M to two decimal places) at equilibrium? A: 5.51 x 10 -15 (2) (028 DES (2)₂0+ (₂),025 = (8)¿025
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While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH, ) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 75 L tank with 5.6 mol of ethylene gas and 7.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 2.3 mol of ethylene gas and 4.4 mol of water vapor. The engineer then adds another 2.8 mol of ethylene, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. ||mol x10
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Consider the reaction: N₂O4 (9) — 2NO2 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: N₂(g) +202 (g) = N₂O4 (9) K₁ 1/2N₂(g) + O2(g) — NO2(g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K=