<8:48Calculating an equilibrium constant from an equilibrium compositionHydrogen and chlorine react to form hydrogen chloride, like this:H₂(g) + Cl₂(g) → 2HCl(g)compound pressure at equilibriumH₂72.7 atmCh₂₂HCI80.2 atmToday8:48 PMAlso, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chlofollowing composition:42.9 atm.5G3EditCalculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digitsKp=€Ep

Given, Reaction : H2(g) +CI2(g) →2 HCI(g)

Calculating an equilibrium constant from an equilibrium composition Hydrogen and chlorine react to form hydrogen chloride, like this: H₂(g) + Cl₂(g) → 2 HCl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chlo following composition: compound pressure at equilibrium 72.7 atm Cl₂ HCI 80.2 atm 42.9 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits 3

Calculating an equilibrium constant from an equilibrium composition Hydrogen and chlorine react to form hydrogen chloride, like this: H₂(g) + Cl₂(g) → 2 HCl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chlo following composition: compound pressure at equilibrium 72.7 atm Cl₂ HCI 80.2 atm 42.9 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits 3

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

See similar textbooks

Similar questions

In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
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.
For a typical equilibrium problem, the value of K and the initial reaction conditions are given for a specific reaction, and you are asked to calculate the equilibrium concentrations. Many of these calculations involve solving a quadratic or cubic equation. What can you do to avoid solving a quadratic or cubic equation and still come up with reasonable equilibrium concentrations?
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)