Complete the following chart by writing "LEFT", "RIGHT" OR "NONE" for equilibrium shift, and "INCREASES", "DECREASES" or "REMAINS THE SAME" for the concentrations of reactants and products when theindicated stressors are applied to the given system at equilibrium.2 SO2 (g) + O2(g) 2 SO3 (g)ConcentrationConcentrationConcentrationStressEquilibrium Shiftof SO2of 02of SO31. Add022.RemoveSO23. AddSO34. AddCl2

Reaction in equilibrium means rate of the forward reaction equals the rate of the reverse reaction.…

Complete the following chart by writing "LEFT", "RIGHT" OR "NONE" for equilibrium shift, and "INCREASES", "DECREASES" or "REMAINS THE SAME" for the concentr indicated stressors are applied to the given system at equilibrium. 2 SO2 (g) + O2(g) 2 SO3 (g) Concentration of S03 Concentration Concentration Stress Equilibrium Shift of S02 of 02 1. Add 02 2. Remove so2 3. Add So3 4. Add Cl2

Complete the following chart by writing "LEFT", "RIGHT" OR "NONE" for equilibrium shift, and "INCREASES", "DECREASES" or "REMAINS THE SAME" for the concentr indicated stressors are applied to the given system at equilibrium. 2 SO2 (g) + O2(g) 2 SO3 (g) Concentration of S03 Concentration Concentration Stress Equilibrium Shift of S02 of 02 1. Add 02 2. Remove so2 3. Add So3 4. Add Cl2

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 mixture of water and graphite is heated to 890 K in a 14.5-L container. When the system comes to equilibrium it contains 0.835 mol each of CO gas and H2 gas and 0.182 mol of H2O gas and some graphite. Some O2 gas is added to the system and a spark is applied so that the H2 reacts completely with the O2, forming H2O. Find the amount of CO in the flask when the system returns to equilibrium.
A 1.0-L container originally holds 0.4 moles of N2, 0.1 moles of O2, and 0.08 moles of NO. If the volume of the container holding the equilibrium mixture is decreased to 0.5 L without changing the quantities of the gases present, how will their concentrations change? State whether each will increase, decrease, or stay the same. N2(g) + O2(g)<->2NO(g)K for the reaction
Nitrogen and hydrogen react to form ammonia, like this: N₂(g) + 3 H₂(g) → 2NH3(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 67.1 atm H₂ NH3 K = P 43.5 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. р 0 83.8 atm x10 X Ś
What is the correct correlation between the graphs and the numbered stresses below for this equilibrium system 2 SO2(g) + O2(g) ⇌ 2SO3 (g) + heat 1. temperature was increased 2. temperature was decreased 3. pressure was increased by decreasing volume 4. pressure was decreased by increasing volume 5. SO3 was added 6. SO3 was removed 7. O2 was added 8. O2 was removed
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
When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to Konce again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K. The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: If a stress is applied to a reaction mixture at equilibrium, a net reaction occurs in the direction that relieves the stress.
Initial (M) Change (M) Equilibrium (M) -2.0 Consider the equilibrium system described by the chemical reaction below. A mixture of gas containing only N₂ and H₂ is reacted in a vessel at high temperature. At equilibrium, the 5.0 M H2, 8.0 M N₂, and 4.0 M NH3 are present. Determine the initial concentrations of H₂ and N₂ that were present in the vessel. Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. 0 2.0 5.0 N₂(g) + 3 H₂(g) = 2 NH3(g) -5.0 N₂(g) Ssivestit 8.0 1 6.0 + 4.0 -6.0 3 H₂(g) ઇસ્કો અને કોની -4.0 10 10.0 2 NH3(g) RESET 11.0
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Decide whether each of the following statements is true or false. If false, change the wording of the statement to make it true. a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction. d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.
Suppose a 500flask is filled with 0.20 mol of fNO_{3} and 0.50 mol of NO_{2} The following reaction becomes possible: NO 3 (g)+NO(g) leftarrow2NO 2 (g) The equilibrium constant K for this reaction is 4.79 at the temperature of the flask Calculate the equilibrium molarity of NO_{3} Round your answer to two decimal places
Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(g)→ 3 NO,(g)+H,0(1) At a certain temperature, a chemist finds that a 4.5 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount dlo HNO3 14.2 g 18 Ar NO 7.3 g NO, 19.2 g H,O 87.0 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 x10 ?