Questions: 1) Using the equilibrium shown below, fill in the table showing which way each stress would shift things to re-establish equilibrium and the effect on the value of Kc each stress will have. Assume that only the stress that is being applied is happening to the system at equilibrium and nothing else changes (e.g. the volume of the container remains constant unless you are told otherwise). 2CHC13(g) +Cl2(g) = 2CCl4(1) + H₂(g) Stress Add Cl₂(g) Add CC140) Remove CHCl3(g) Cool System Add a catalyst Reduce volume Add He(g) ΔΗ = .60 kJ Direction of shift to re- establish equilibrium 93 ΔΗ = 130 kJ Change in the value of Kc 2) For the equilibrium shown below, list three things that you could do to decrease the yield of the products. H₂O(g) + C(s) = CO(g) + H₂(g)

Questions: 1) Using the equilibrium shown below, fill in the table showing which way each stress would shift things to re-establish equilibrium and the effect on the value of Kc each stress will have. Assume that only the stress that is being applied is happening to the system at equilibrium and nothing else changes (e.g. the volume of the container remains constant unless you are told otherwise). 2CHC13(g) +Cl2(g) = 2CCl4(1) + H₂(g) Stress Add Cl₂(g) Add CC140) Remove CHCl3(g) Cool System Add a catalyst Reduce volume Add He(g) ΔΗ = .60 kJ Direction of shift to re- establish equilibrium 93 ΔΗ = 130 kJ Change in the value of Kc 2) For the equilibrium shown below, list three things that you could do to decrease the yield of the products. H₂O(g) + C(s) = CO(g) + H₂(g)

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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QUESTION 4 For the following system at equilibrium, predict whether the reaction will shift to the right, left, or not be affected by a decrease in temperature. Also, determine the value of the equilibrium constant increase or decreases. PCl5(g) ⇌ PCl3(g) + Cl2(g) endothermic The reaction will shift to the left and the K value will increase. The reaction will shift to the right and the K value will decrease. The reaction will not be affected and the K value does not change. The reaction will shift to the left and the K value will decrease. The reaction will shift to the right and the K value will increase.
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Question 1 State the direction that the equilibrium will shift in response to each stress applied to this chemical reaction that produces carbonic acid: .CO2 (g) + H2O (I) = H2CO3 (aq) Additional water is added. [Choose ] Some carbonic acid is removed. [ Choose ] The pressure of the container is decreased. [ Choose ] The temperature is increased. [Choose ] > >
Consider the following equilibrium system: 2 NOCI(g) 2 2 NO(g) + Cl2(g) Kc = 57.0 Initially, only NOCI gas is placed in a flask. After equilibrium has been reached it is found that the concentration of the nitrogen monoxide gas in the flask is 1.14 mol/L. What is the initial molar concentration of the NOCI gas? Answer to three decimal places.
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1.QuestionGiven the reaction at equilibrium: 2 SO2(g) + O2(g) <--> 2 SO3(g) + heat Which change will shift the equilibrium to the right? increasing the temperature increasing the pressure decreasing the amount of SO2(g) decreasing the amount of O2(g)
Consider a reaction A21g2 + B21g2 ∆ 2 AB1g2, with atoms of A shown in red in the diagram and atoms of B shown in blue. (a) If Kc = 1, which box represents the system at equilibrium?
QUESTION 5 The reduction of iron (II) oxide, FeO by carbon monoxide, CO to produce iron and carbon dioxide, COz is according to the equation below. FeO (s) + CO (g) = Fe (s) + CO2 (g) initially, 0.500 mol of CO was allowed to react with FeO in a sealed container at a certain temperature. The total pressure at equilibrium is 1.5 atm. Calculate the equilibrium partial pressures of CO (g) and CO2 (g).
Consider the following equilibrium: 2 NH3(g) N2 (g) + 3 H2(g) Which of the following will happen when nitrogen gas (N₂) is added to the reaction mixture? --> The concentration of NH3 will decrease. The value of Keq will increase. The value of Keq will decrease. The concentration of H₂ will decrease.
QUESTION 2 The following equilibrium process has been studied at 230°C: 2NO(g) + O2(g) - 2NO2(g) In one experiment, the concentrations of the reacting species at equilibrium are found to be [NO] = 0.0542 M, [02] = 0.127 M, and [NO2] = 15.5 M. Calculate the equilibrium constant (Kc) of the reaction at this temperature. Note: Express your final answer in scientific notation. Round off into 2 decimal places. Example: 1.11 x 10 or 1.11 x 10^(-11)