University:
College of Central Florida
Course:
CHM2046 | General Chemistry II
Academic year:

2024
Views:

99

Pages:

14
Author:

Altenopoots7okd

Chemistry 12 Chemistry 12 Unit 2-Chemical Equilibrium Worksheet 2-3 KEY Calculations Involving the Equilibrium Constant Keq) 1. Given the equilibrium equation below: A2(g)+ B2(g)2AB() If, at equilibrinon, the concentrations are as follows: 2SD [A-3.45 M. [B2]-5.67 M and [AB]-0.67 M a) Write the expression for the equilibrium constant, Keq 2 ΣΑΒΙ [A23 [B2] b) Find the value of the equilibrium constant, Keg at the temperature that the experiment was done. 2 Keg (0.67) (3.45)(5.67) 0.023 Answer Kez. = 0.023 2. Given the equilibrium equation: X2g)+ 3Y2)2XY3(g) at a temperature of 50°C, it is found that when equilibrium is reached that: [X2]=0.37 M. [2]-0.53 M and [XY]-0.090 M (All 2 SD) a) Write the equilibrium constant expression (Keq) Keg [XY3] 2 [X] [Y] b) Calculate the value of Keq at 50°C. (0.090)2 Keg (0.37) (0.53)3 = 0.15 Answer Kez = 0.15 Worksheet 2-3 Calculations Involving the Equilibrium Constant Page 1 Chemistry 12 Unit 2-Chemical Equilibrium 3. For the reaction: A2(g) B(g) 20(g) KEY it is found that by adding 1.5 moles of C to a 1.0 1. container, an equilibrium is established in which 0.30 moles of B are found. (Hint: Make a table and use it to answer the questions below) 2/1 Idec place [I] A2 + B 0 1.5 0 +0.30 -0.60 [C] +0.30 0.30 0.30 2 C 0.9 کے [E] a) What is [A] at equilibrium? Answer 0.30M b) What is [B] at equilibrium? Answer 0.30 M c) What is [C] at equilibrium? Answer 0.9 M = d) Write the expression for the equilibrium constant, Ke 2 Keq = [C] ΣΑΙ [Β] e) Calculate the value for the equilibrium constant at the temperature at the experiment was done. ISD Keg = (0.9) (0.30) (0.30) 9 Answer Keq=9 Worksheet 2-3 Calculations Involving the Equilibrium Constant Page 2 Chemistry 12 20. Given the equilibrium equation: KEY Unit 2-Chemical Equilibrium 3A(g)+B(g) 20(g) If 2.50 moles of A and 0.500 moles of B are added to a 2.00 1. container, an equilibrium is established in which the [C] is found to be 0.250 M. Initial [A]=2.50mal-1.25M [B]=0.500mal 2.001 a) Find [A] and [B] at equilibrium. 3/2 3A+B 2C 1.25 0.250 [ C]-0.375-0.125 +0.250 E 0.875 0.125 4 2 dec. ploces 0.250 Answer [A]=0.88M [B]=0.125 M 2.00L 0.250M b) Calculate the value of the equilibrium constant Keq Keg = [C]² = (0.250)² [A] [B] (0.875)3 (0.125) = 0.746 Answer Keq = 0.75 21. At 800°C, the equilibrium constant Keq, for the reaction: CO2(g)+ H2(g)CO(g) H10(g) is 0.279 If 1.50 moles of CO2 and 1.50 moles of H₂ are added to a 1,00 L. container, what would the [CO] be at equilibrium? Keg = [CO][H₂O] CO₂+ H₂CO + H₂O 2 70.7423-0,5282× =X [CO2] [H2] [1] 1.50 1.50 [C] -X -x +x 0 0.279 x 2 0.7923=1.5282x +x (1.50-x)2 x=0.7923 [E] 1.50-x 1.50-к X V0.279 メ 1.5282 [E] 1.50-0,5185 1.50-0.5185 0.5185 0.5185 [E] 0.982 0.982 0.518 0.518 0.5282(1.50-x) = x Answer equilm [CO3 = 0.518 M 1.50-x x=0.5185 Worksheet 2-3-Calculations Involving the Equilibrium Constant Page 11

Calculation involving equilibrium constant

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