1. For the reaction below: PC13(g) + Cl2(g) PC15(g) When a particular reaction is started, it is 0.410 M in PC13 and 0.107 M in C2. When this reaction reaches equilibrium, it contains 0.0250 M PCI5. Generate an ICE chart for this reaction, and indicate the concentration of all compounds at equilibrium. Also, find the value of K.

1. For the reaction below: PC13(g) + Cl2(g) PC15(g) When a particular reaction is started, it is 0.410 M in PC13 and 0.107 M in C2. When this reaction reaches equilibrium, it contains 0.0250 M PCI5. Generate an ICE chart for this reaction, and indicate the concentration of all compounds at equilibrium. Also, find the value of K.

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

6. You are given the following equation: A₂B2A + B) You fill a 1 L flask with 0.20 mol of A2B 0.5% of this substance dissociates. What is the value of K? 7.5.6 x 10-6 mol of A and 5 x 10¹5 mol of B are mixed in a 200 mL flask. The system is represented by the equation 2A + B = 30 At equilibrium, there is 4.8 x 105 mol of B. Calculate the value of the equilibrium constant 8 K=1.7 x 10-10 for the following system which represents the dissolving of silver chloride AgCl) Ag*(a) + Cl (2) What will the concentration of Ag* be at equilibrium (in M)? 9. You work with the following system: 2X=Yu At equilibrium, [Y]-3[X] If K=10, calculate the [Y] at equilibrium.
Part A A sample of pure NO2 is heated to 334 °C at which temperature it partially dissociates according to the equation 2 NO2 (g) = 2 NO (g) + O2 (g) At equilibrium the density of the gas mixture is 0.520 g/L at 0.750 atm . Calculate K. for the reaction. Π ΑΣφ. K = .0133 Submit Previous Answers Request Answer Incorrect; Try Again; 3 attempts remaining
Calculate Equilibrium Concentrations (from Initial concentrations and K): Hydrogen gas can be produced in several different ways. The following reaction illustrates one method using carbon monoxide and water: CO(g) + H2O(g) ⇌ H2(g) + CO2(g) At 700 K the equilibrium constant is 0.83. If you start 1.0 mol CO(g) and 1.0 mol H2O(g) in a 5.0 dm3 container, what amount of each substance will be present when the gases are in equilibrium.
9. Consider the reaction: 2 A (g) + 3 B (g) = 2 C (g) + 4 E (g). The reaction is initiated with 0.60 M in A, 0.45 M in B and 0.50 M in E (Note 0 M in C). At equilibrium, the value of [B] = 0.15 M. What is the equilibrium value of [E]? a) 0.95 M b) 0.90 M c) 0.80 M d) 0.60 M e) 0.50 M f) 0.40 M g) none of the above 0 4 15 Determine the acid ionization constant
19.26 Draw the structure of the sphingolipid containing palmitic acid and a-D-glucose.
3. A 13.0 Liter flask at 499 °C contained 0.852 mole of hydrogen, 0.361 mole of I₂ and 3.84 mol of HI. Assuming that the substances are at equilibrium, find the value of K. at this temperature for the reaction: H₂(g) + L₂(g) 2HI (g)
Help me !!!
Consider the equilibrium reaction. H₂(g) + 1₂(9) ⇒ 2 HI(g) In this case, 1.000 M H₂ reacts with 2.000 M of 1₂ at a temperature of 430.ºC. The value of K = 68. Determine the equilibrium concentrations of H₂, I₂, and HI. C M [H₂] [1₂] M [HI] M
7. Ammonia can be synthesized according to the equation: 1/2 N₂(g) + 3/2 H₂(g) → NH3(g). The equilibrium constant is 1.69 x 10-4 at 673 K and AHO is -106.5 kJ mol-¹. Calculate the equilibrium constant at 773 K.
CO(g) + H₂O(g) ⇒ H₂(g) + CO₂(g) K = 7.3@823 K A closed 5.0 L container initially holds 3.0 moles CO and 6.0 moles H2O. Calculate the concentrations of each material at equilibrium. What is the equilibrium concentration of H₂O? [H₂O] = [?] M
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.
6. Give the equilibrium constant for the following reaction. 2PB1, (g) + 3Cl,(s) 2PCI;(g) + 3Br,(g)