3. Using ICE Table. The reversible reaction: 2SO2 + Oze) 2SO3 has come to equilibrium in a vessel of specific volume at a given temperature. Before the reaction began, the concentrations of the reactants were 0.060 M of SO2 and 0.050 M of O2. After equilibrium is reached, the concentration of SO3 is 0.040 M. What is the equilibrium concentration of O2? 4 Using ICE Table, consider the reaction PCl3@ + Cl2@ - PClse Ke= 0.040 at 450°C. If a reaction is initiated with 0.40 mole of Cl2 and 0.40 mole of PCl3 in a 2.0 liter container, what is the equilibrium concentration of PCl; in the same system?

3. Using ICE Table. The reversible reaction: 2SO2 + Oze) 2SO3 has come to equilibrium in a vessel of specific volume at a given temperature. Before the reaction began, the concentrations of the reactants were 0.060 M of SO2 and 0.050 M of O2. After equilibrium is reached, the concentration of SO3 is 0.040 M. What is the equilibrium concentration of O2? 4 Using ICE Table, consider the reaction PCl3@ + Cl2@ - PClse Ke= 0.040 at 450°C. If a reaction is initiated with 0.40 mole of Cl2 and 0.40 mole of PCl3 in a 2.0 liter container, what is the equilibrium concentration of PCl; in the same system?

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...

See similar textbooks

Similar questions

Picture 1 is A) And Picture 2 is B)
Consider the equilibrium reaction below: N₂(g) + O₂(g) 2 NO(g) Create an equilibrium constant, K, expression for the above reaction using the drag and drop tools: K= [N₂][0₂] [N₂]+[0₂] [NO]² [N]²[O]² [NO] 2[NO]
URGENT PLEASE ANSWER THE FOUR QUESTION THE CHOICES IS THE 2ND PICTURE
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 7.1 × 10⁻⁴ at a certain temperature. If a solid sample of CaCrO₄ dissolves in solution, what will the equilibrium concentration of Ca²⁺ in the solution be? Based on the given values, set up ICE table in order to determine the unknown Based on your ice table, set up the expression Kc Based on your ice table and expression for Kc, solve for the concentration Ca2+ at equilibrium
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x
The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500K.PCl5(g) PCl3(g) + Cl2(g)If an equilibrium mixture of the three gases in a 13.6 L container at 500K contains 0.230 mol of PCl5(g) and 0.374 mol of PCl3, the equilibrium concentration of Cl2 is M.
Equilibrium constant, Kc, for the following reaction is 8.08×10-3 at 1080 K.2SO3(g) 2SO2(g) + O2(g)Calculate the concentration of SO3 in the equilibrium mixture?When a sufficiently large sample of SO3(g) is introduced into an evacuated vessel at 1080 K, the equilibrium concentration of O2(g) is found to be 9.70×10-2 M.
MAI Van JL.cas-Cudo Lab Assignment #3 E.mheducation.com Saved # 3 6 Be sure to answer all parts. Consider the following equilibrium system involving SO2, Cl2, and SO,Cl, (sulfuryl dichloride): SO2(g) + Cl2(g) = SO,C(g) Predict how the equilibrium position would change if the following changes were to occur. The temperature remains constant in each case. (a) Cl, gas is added to the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. ((More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (b) SO,Cl, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (c) SO, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More…
Question 29 of 30 Consider the reaction of N2O and O2 described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 NO(g) +3 O₂(g) 4 NO2(g) 1 2 NEXT > A 1.00 L reaction vessel was filled with 0.0560 mol O2 and 0.200 mol N2O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. 2N₂O(g) + 302(g) == 4NO2(g) Initial (M) 0.200 -0.0100 0.190 Change (M) 0.0560 -0.0150 0.0410 Equilibrium (M) 0 0.0200 0.0200 RESET 0 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190
6. Hydrogen gas is finding more acceptance as an alternative fuel. It is produced along with carbon dioxide by the reaction of carbon monoxide and gaseous water at 915 K. At this temperature, the equilibrium constant (K.) is 1.56. If this reaction is started in a 4.00 L closed system flask with 0.450 mol of CO, 1.25 mol H2O, 1.15 mol CO2, and 3.50 mol H2, calculate the concentrations of all substances in the flask initially and at equilibrium. Put these values in the ICE table below. (Hint: you will need to use the quadratic formula.) CO Н20 CO2 H2 INITIAL CHANGE EQUILIBRIUM 0.1125 0.3125 0.2875 0.875 -X -X +X +x e these values in the table. d. Calculate the reaction quotient, Q. e. Express the direction of equilibrium shift as an algebraic expression. Complete the change row of the table. f. Substitute the algebraic expressions into the equilibrium expression and solve for the equilibrium concentrations. Place these values in the table.
Consider the equilibrium system described by the chemical reaction below. Determine the concentration of O, at equilibrium by writing the equilibrium constant expression and solving it. Complete Parts 1-2 before submitting your answer. = 2 H₂O(g) 2 H2(g) + O̟₂(g) 1 2 NEXT At this temperature, the Kc = 2.4 × 103 and the equilibrium concentrations of H2O and H2 are 0.11 M and 0.019 M, respectively. If [x] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Кс = 2' = 2.4 × 103 > RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11]² [0.019]² [x] [x]² [2x] [2x]²
2) At 250°C, the equilibrium constant (Kc) for the reaction given below is 1.80. PCIS(g) PC13(g) + Cl2(g) Some PCI5 is placed in a reaction vessel and the contents maintained at a temperature of 250ºC and allowed to achieve equilibrium. The equilibrium concentration of PCI5 is 0.28 M Calculate the equilibrium concentration of PCI3 and C12