Calculating an equilibrium constant from an equilibrium composition Hydrogen and chlorine react to form hydrogen chionde, like this: H₂(g) + Cl₂(o)- 2HCl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chloride has the following composition: compound pressure at equilibrium H₂ 72.7 atm Cl₂ HCI 80.2 atm 42.9 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. -Interran

Calculating an equilibrium constant from an equilibrium composition Hydrogen and chlorine react to form hydrogen chionde, like this: H₂(g) + Cl₂(o)- 2HCl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chloride has the following composition: compound pressure at equilibrium H₂ 72.7 atm Cl₂ HCI 80.2 atm 42.9 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. -Interran

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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Chlorine and water react to form hydrogen chloride and oxygen, like this: 2 Cl₂(g) + 2 H₂O(g) → 4 HCl(g) + O₂(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of chlorine, water, hydrogen chloride, and oxygen has the following composition: compound pressure at equilibrium C1₂ 42.2 atm H₂O 95.0 atm HC1 78.1 atm 0₂ 47.1 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K₂= 0 3 ? 0x10
Mercury and oxygen react to form mercury(II) oxide, like this: At a certain temperature, a chemist finds that a 4.0 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: 2 Hg(1)+O,(g)→2 HgO(s) compound amount 22.1 g Hg O2 24.2 g HgO 19.5 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N,(g) + 2 H,O(g) 2 NO(g) + 2 H,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition: compound pressure at equilibrium N2 27.4 atm H,O 22.7 atm NO 51.8 atm H, 91.7 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = | Submit Assignmer Continue MacBook Air 80 F3 888 F4 F6 F2 $ % & 6 7 8 9
Mercury(II) oxide decomposes to form mercury and oxygen, like this: 2 HgO(s)→2 Hg(1)+O2(g) At a certain temperature, a chemist finds that a 3.3 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the following composition: compound amount HgO 19.5 g Hg 14.6 g O2 0, 17.4 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 x10
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Nitrogen and hydrogen react to form ammonia, like this: N,(g) + 3 H,(g) → 2 NH,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, hydrogen, and ammonia has the following composition: compound pressure at equilibrium N2 82.3 atm H2 38.7 atm NH3 73.0 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits.
Hydrogen and chlorine react to form hydrogen chloride, like this: H,(g) + Cl,(g) → 2 HCl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chloride has the following composition: compound pressure at equilibrium H2 20.2 atm Cl 2 50.0 atm HC1 7.95 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. р K 4 x10
For the chemical equation: SO2(g) + NO2(g) SO3(g) + NO(g) The equilibrium constant at a certain temperature is 8.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 6.20 mol SO2(g) in order to form 4.40 mol SO3(g) at equilibrium.
Calcium oxide and carbon dioxide react to form calcium carbonate, like this: CaO(s)+CO2(g)→CaCO3(s) At a certain temperature, a chemist finds that a 4.4 L reaction vessel containing a mixture of calcium oxide, carbon dioxide, and calcium carbonate at equilibrium has the following composition: compound amount Cao 31.2 g CO2 16.8 g CACO3 32.3 g Calculate the value of the equilibrium constant K̟ for this reaction. Round your answer to 2 significant digits. K = [| Submit A Continue MacBook Air F10
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Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4(9) +20 2(g) =CO2(g) + 2H 20(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is reduced? O a. The equilibrium position is shifted to the left and the value for K increases. O b. The equilibrium position is shifted to the right and the value for K increases. O c. The equilibrium position is shifted to the right and the value for K decreases. O d. The equilibrium position is shifted but the value for K stays constant. Oe. The equilibrium position is shifted to the left and the value for K decreases.
When nitrogen gas reacts with oxygen gas, nitrogen monoxide gas forms: N2(g) + O2(g) ⇋2NO(g) Initially, 0.40 mol of each reactant is placed into a 2.0 L container and equilibrium is established. If Keq=50.1 for the reaction, what are the equilibrium concentrations of all reactants and products? What two conditions are required, if we want to move reaction forward.