(a)
Interpretation:
The effect of equilibrium has to be explained, after the addition of Chlorine into Phosphorus pentachloride decomposition reaction.
Concept Introduction:
Le Chatelier's principle:
Le Chatelier's principle states that if a system in equilibrium gets disturbed due to modification of concentration, temperature, volume, and pressure, then it reset to counteract the effect of disturbance.
The concentrations of reactant and product are equal in equilibrium
(b)
Interpretation:
The effect of equilibrium has to be explained, after the addition of Phosphorus trichloride into Phosphorus pentachloride decomposition reaction.
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The effect of equilibrium has to be explained, after the addition of Phosphorus pentachloride into Phosphorus pentachloride decomposition reaction.
Concept Introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 12 Solutions
Chemistry: The Molecular Science
- How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.arrow_forwardExplain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates are equal.arrow_forwardA student adds 0.600 mol of methane gas, CH4(g) into a 2.00 L container and the methane forms ethyne, C2H2(g) and hydrogen gas, H2(g). At equilibrium, the container was found to contain 0.045 mol/L C2H2.a) Calculate the initial concentration of CH4. Then complete an ICE Table to organize the initial, change and equilibrium concentrations for this equilibrium system. Show any calculations needed. 2CH4(g) ⇄ C2H2(g) + 3H2(g)b) Calculate the equilibrium constant, Keq, for this equilibrium. Show all work.c) What is the equilibrium concentration of H2(g) ?arrow_forward
- What is meant by the term “chemical equilibrium”? Must amounts of reactants and products be equal at equilibrium?arrow_forwardThe graph below shows the concentration of reactants and products in a chemical reaction that reaches equilibrium. Explain, from the graph, what is happening to the concentration of reactants and products before and after equilibrium is reached.arrow_forwardAs we continue to explore equilibrium, it is important that we look at LeChatelier's Principle. This simple idea, if we disturb a system in chemical equilibrium, the reaction will shift to reestablish equilibrium, is incredibly useful in many manufacturing processes. Consider a chemical process to manufacture a specific substance. When it reaches equilibrium, and there are still reactants available, if we remove the product(s) the reaction will move towards the products until it reaches equilibrium again. In theory we can push a reaction to use up all reactants by removing the product to interrupt equilibrium.arrow_forward
- In general, for a system at equilibrium, indicate the direction the equilibrium will shift for the following change. The concentration of one or more of the products is increased.arrow_forwardWhat property of a reaction can we use to predict the effect of a change in temperature on the value of an equilibrium constant?arrow_forwardDefine the term Equilibrium Constant?arrow_forward
- Assume that the following endothermic chemical reaction is at equilibrium. C(s) + H₂O(g) + H₂(g) + CO(g) Which of the following statements is/are CORRECT? 1. Increasing the concentration of H₂(g) will cause the reaction to proceed in the backward direction, increasing the equilibrium concentration of H₂O(g). 2. Decreasing the temperature will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). 3. Increasing the amount of C(s) will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). All statements are correct. 2 only 3 only 1 only 1 & 2 onlyarrow_forwardConsider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningLiving By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
- Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co