Homework 4 Question 9 of 30 (1 point) | Question Attempt: 1 of 3 ✓ 2 ✓ 3 ✓ 4 ✓ 5 6 ✓ 7 ✓ 8 = 9 10 11 Given this reaction at 25 °C. PCl5(g) = PC13(g) + Cl₂ (g) Compound Cl₂ (g) PCl₂ (g) PC15 (g) Initial Partial Pressure(atm) 0.306 0.234 0.00330 Use the table of initial partial pressure to find: Note: Reference the Thermodynamic properties of pure substances and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 1 significant digit. Кр = 21.7 ப x10 Part 2 of 2 ☑ Round your answer to 3 significant digits. Check AG = -7.628 kJ mol ☐ x10 ☐ Save For Later Subr

Homework 4 Question 9 of 30 (1 point) | Question Attempt: 1 of 3 ✓ 2 ✓ 3 ✓ 4 ✓ 5 6 ✓ 7 ✓ 8 = 9 10 11 Given this reaction at 25 °C. PCl5(g) = PC13(g) + Cl₂ (g) Compound Cl₂ (g) PCl₂ (g) PC15 (g) Initial Partial Pressure(atm) 0.306 0.234 0.00330 Use the table of initial partial pressure to find: Note: Reference the Thermodynamic properties of pure substances and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 1 significant digit. Кр = 21.7 ப x10 Part 2 of 2 ☑ Round your answer to 3 significant digits. Check AG = -7.628 kJ mol ☐ x10 ☐ Save For Later Subr

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section15.6: Disturbing A Chemical Equilibrium

Problem 1RC: The formation of ammonia from its elements is an important industrial process. 3 H2(g) + N2(g) 2...

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A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.
Consider the formation of HI(g) from H2(g) and I2(g). H2(g)+I2(g)2HI(g) For this reaction, K at 333C is 98, while K at 527C is 62.5. Find S for I2(g) at 527C.
Data in the table were collected at 540 K for the following reaction: CO(g) + NO2(g) CO2(g) + NO(g) Using the data in the table: (a) Determine the reaction order with respect to each reactant. (b) Derive the rate equation. (c) Calculate the rate constant, giving the correct units for k.
Sodium sulfate 10-hydrate, Na2SO410H2O, dehydrates according to the equation Na2SO410H2O(s)Na2SO4(s)+10H2O(g)KP=4.081025 at 25 C What is the pressure of water vapor at equilibrium with a mixture of Na2SO410H2O and NaSO4?
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Consider the following reaction at some temperature: H2O(g)+CO(g)H2(g)+CO2(g)K=2.0 Some molecules of H2O and CO are placed in a 1.0-L container as shown below. When equilibrium is reached, bow many molecules of H2O, CO, H2, and CO2 are present? Do this problem by trial and error-that is, if two molecules of CO react, is this equilibrium; if three molecules of CO react, is this equilibrium; and so on.
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
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