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For which K= 130.0.Assume that 0.406 mol C (g) is placed in a cylinder. The Temperature is 300.0 K,and the barometric pressure on the piston (which is assumed to be massless and frictionless is constant at 1.00 atm. The original volume (before the 0.406 mol C(g) begins to decompose is 10.00 L) .What is the volume in the cylinder at equilibrium ?

For which K= 130.0.Assume that 0.406 mol C (g) is placed in a cylinder. The Temperature is 300.0 K,and the barometric pressure on the piston (which is assumed to be massless and frictionless is constant at 1.00 atm. The original volume (before the 0.406 mol C(g) begins to decompose is 10.00 L) .What is the volume in the cylinder at equilibrium ?

Chemistry
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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Date due: A (g) + B (g) → C (g) For which K= 130.0.Assume that 0.406 mol C (g) is placed in a cylinder.The Temperature is 300.0 K, and the barometric pressure on the piston (which is assumed to be massless and frictionless is constant at 1.00 atm. The original volume (before the 0.406 mol C(g) begins to decompose is 10.00 L) .What is the volume in the cylinder at equilibrium ? Consider the reaction a Do the total moles increae or decrease? WHY? & use b Does the volume increase or decrease? WHY? 2)₁ The pressure total is 1.00 atm.Use this knowledge to check your answer after you have calculated V at equilibrium. Pay attention $14-10 1. Solve for concentrations of A,B, and C assuming volume remains at 10.00 L using the quadratic equation. 2. Solve for total moles at equilibrium to get the final volume.Remember the Ideal Gas Law Equation-what is held constant ?How are total moles and total volume related ? 3. Solve for V.Be sure to relate the equilibrium concentrations to the new volume V at equilibrium.Substitute V from ideal equation into K expression to solve for V. 4. Then check to see if K=130 and P total = 1.00 atm Additional 2 BONUS points can be earned by determining the volumes by successive approximations to approximate the final pressure which will be 1.00 atm.HINT use BOYLe's LAW.
Transcribed Image Text:Date due: A (g) + B (g) → C (g) For which K= 130.0.Assume that 0.406 mol C (g) is placed in a cylinder.The Temperature is 300.0 K, and the barometric pressure on the piston (which is assumed to be massless and frictionless is constant at 1.00 atm. The original volume (before the 0.406 mol C(g) begins to decompose is 10.00 L) .What is the volume in the cylinder at equilibrium ? Consider the reaction a Do the total moles increae or decrease? WHY? & use b Does the volume increase or decrease? WHY? 2)₁ The pressure total is 1.00 atm.Use this knowledge to check your answer after you have calculated V at equilibrium. Pay attention $14-10 1. Solve for concentrations of A,B, and C assuming volume remains at 10.00 L using the quadratic equation. 2. Solve for total moles at equilibrium to get the final volume.Remember the Ideal Gas Law Equation-what is held constant ?How are total moles and total volume related ? 3. Solve for V.Be sure to relate the equilibrium concentrations to the new volume V at equilibrium.Substitute V from ideal equation into K expression to solve for V. 4. Then check to see if K=130 and P total = 1.00 atm Additional 2 BONUS points can be earned by determining the volumes by successive approximations to approximate the final pressure which will be 1.00 atm.HINT use BOYLe's LAW.
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