5. Consider a general reversible reaction: A+B- X+Yand answer the following questions.a. Describe what happens at equilibrium in terms of reaction rate and chemical concentrations?b. Write the expression for the equilibrium constant for the given reaction.6. Consider the following general reversible reaction is taking place in a reaction vessel andhas achieved a state of chemical equilibrium.A+2B 2XIf the following stresses are applied to this reaction at equilibrium, which direction (forward orbackward) will the equilibrium shift?a. Increase in concentration of AB. Decrease in concentration of XFactors Affecting Reaction Rate, Chemical Equilibrium and Le Chatelier'sPrincipleMAYtv

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and answer the following questions. a. Describe what happens at equilibrium in terms of reaction rate and chemical concentrati b. Write the expression for the equilibrium constant for the given reaction. 6. Consider the following general reversible reaction is taking place in a reaction vessel ar has achieved a state of chemical equilibrium. 2X A+2B.

and answer the following questions. a. Describe what happens at equilibrium in terms of reaction rate and chemical concentrati b. Write the expression for the equilibrium constant for the given reaction. 6. Consider the following general reversible reaction is taking place in a reaction vessel ar has achieved a state of chemical equilibrium. 2X A+2B.

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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3. Phosgene gas decomposes according to the following reaction. If a sample of phosgene gas at an initial concentration of 0.500 M is heated at 527°C in a reaction vessel, the concentration of carbon monoxide at equilibrium is 0.046 M. Calculate the equilibrium constant for the reaction at 527°C. COCl2(g) CO(g) + Cl2(g) + 4. The equilibrium constant for the following equation is Kc = 0.11. Calculate the equilibrium concentrations of ICI (g), 12(g), and Cl2(g) when 0.65 moles of 12(g) and 0.33 moles of Cl2(g) are mixed in a 1.5-liter reaction vessel. 2 ICI(g) 12(g) + Cl2(g)
= ◇ KINETICS AND EQUILIBRIUM Calculating an equilibrium constant from a heterogeneous... Calcium carbonate decomposes to form calcium oxide and carbon dioxide, like this: CaCO3(s) → CaO(s) + CO₂(g) At a certain temperature, a chemist finds that a 6.4 L reaction vessel containing a mixture of calcium carbonate, calcium oxide, and carbon dioxide at equilibrium has the following composition: compound amount CaCO3 60.7 g CaO 46.5 g CO₂ 6.1 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 0 3/5 3
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Consider the reaction below at a particular temperature: CO2(g) + H2(g) CO(g) + H2O(g) When the reaction has finally reached equilibrium, O the concentrations of all reactants and products will remain constant. O the concentration of CO will be equal to the concentration of CO2. O only the forward reaction will be taking place. O adding a catalyst will cause more products to form
Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed? a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases
At 1000°C water vapor decomposes into hydrogen gas and oxygen gas. The equilibrium constant for this process is 7.3 x 10-18. a. If 1.00 mol of water was placed in a 10.0 L flask, what are the concentrations of each species when the system reaches equilibrium?
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= O KINETICS AND EQUILIBRIUM Using Le Chatelier's Principle to predict the result of changing... Acetylene and oxygen react to form carbon dioxide and water, like this: 2C₂H₂(g) +50₂(g) → 4CO₂ (g)+2H₂O(g) Suppose a mixture of C₂H₂, O₂, CO₂ and H₂O has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation Some H₂O is removed. Some C₂H, is added. change in composition The pressure of C₂H₂ will The pressure of O₂ will The pressure of O₂ will The pressure of CO₂ will ? ? ? ? ? V go up. go down. not change. shift in equilibrium O to the right to the left x O (none) 3/5 to the right to the left (none)
Consider the following reaction equilibrium . PCI3(g) + Cl2(g) PCI5(g) For this reaction, Kc=2.5 x 10-4. Suppose you set up a mixture with each reactant at 4.5 M. In the space below, give the concentration of product at equilibrium. In your uploaded work, give the concentrations of each reactant at equilibrium.
For the reaction: COCI2 (g) + CO + Cl2 (g) (g) At 100°C the reaction has an equilibrium constant of 2.2 x 10-10, If 1.00 mole of phosgene (COCI2) is placed in a 10.0 L flask, calculate the concentration of carbon monoxide at equilibrium. Write your answer in standard form (not scientific notation).
Catalysts affect reaction rates, but do not change either the equilibrium or the spontaneity of a reaction. True or False.
2. Please don't write on a paper. I can't understand handwritten.