When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to K once again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K. The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: If a stress is applied to a reaction mixture at equilibrium, a net reaction occurs in the direction that relieves the stress.

When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to K once again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K. The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: If a stress is applied to a reaction mixture at equilibrium, a net reaction occurs in the direction that relieves the stress.

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

Related questions

Q: ulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: 2. Consider the reaction CO(g) CH3OH(g) 2H2(g) A reaction mixture in a 1.00L flask initially only…

A: Initial concentration of CO and H2 and also the concentration of CH3OH at equilibrium can be…

Q: Nitrogen and hydrogen react to form ammonia, like this: N2(g)+3H,(9) 2 NH3(g) The reaction is…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: Hydrogen and fluorine react to form hydrogen fluoride, like this: H₂(g) + F₂(g) → 2 HF (g) The…

A: Le Chatelier's principle:According to the Le Chatelier's principle when a change in concentration…

Q: The equilibrium constant, K., for the following reaction is 9.52×10-2 at 350 K. CH (g) + CCl, (g)=2…

Q: Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: Chlorine and water react to form hydrogen chloride and oxygen, like this: 2 Cl₂(g) + 2 H₂O(g) → 4…

Q: Ammonia and oxygen react to form nitrogen and water, like this: 4NH3(g)+30₂(g) → 2N₂(g) + 6H₂O(g)…

A: Le-Chatelier's principle:According to the Le Chatelier's principle when a change in concentration…

Q: A chemical engineer is studying the following reaction: 4 HCl(g)+O2(9) → 2 H,O(g)+2C12(9) At the…

A: Given : Balanced equation of hydrochloric acid and oxygen gas. To find : expected changes in…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

A: Information about the question

Q: A chemical engineer is studying the following reaction: HCH;CO,(aq)+CH,NH,(aq) → CH,CO,(aq)+CH,NH…

Q: Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its…

Q: Calcium oxide and carbon dioxide react to form calcium carbonate, like this: CaO(s)+CO,(g)→CaCO;(s)…

A: Complete solution is given below in next step

Q: What does it mean when K>1, K<1, K=1, and when K=0. Is your equilibrium constant always constant,…

A: For a general reaction aA +bB -<------> cC +dD The expression for equilibriumconstant is…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: Hydrogen and fluorine react to form hydrogen fluoride, like this: H₂(g)+F₂(g) → 2 HF (g) The…

A: We have been given perturbations in given table and we have been asked to complete table. Exothermic…

Q: Consider the general reaction 2A(9) + B(s) = C(9) + 3D(9) AH = +115 kJ which has already come to…

A: for the c question the reaction equilibrium shift towards the left direction because for the…

Q: Ammonia and oxygen react to form nitrogen and water, like this: 4NH, (g)+30,(g) 2N, (g)+6H,0(g)…

A: According to Le chatelier principle, equilibrium will shift in such way that counteracted upon…

Q: Limestone, or calcium carbonate, CaCO3(s), decomposes and forms quicklime, CaO(s), and carbon…

A: Given reaction is, CaCO3(s) ⇋ CaO(s) + CO2(g)

Q: A chemical engineer is studying the following reaction: HCH,CO,(aq)+CH,NH,(aq) →…

A: For the reaction given above, CH3COOH (aq) + CH3NH2 (aq) →CH3COO- (aq) + CH3NH3+(aq) We know that,…

Q: Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl,(g)…

Q: The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) PCl5(g)…

A: Given data: PCl3(g)+Cl2(g)→PCl5(g) The equilibrium constant,Kc=83.3 Initial moles of PCl3=0.260 and…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

A: The equilibrium reaction between sulfur dioxide and oxygen to form sulfur trioxide is as follows:…

Q: osphorus pentachloride decomposes according to the chemical equation PCI,(g) = PCI,(g) + Cl,(g) K. =…

A: Given : We have to calculate the equilibrium concentration of PCl5(g) and PCl3(g).

Q: Hydrogen and fluorine react to form hydrogen fluoride, like this: H,(9)+F,(9) → 2 HF(g) The reaction…

A: According to Le Chatelier's Principle : If a system at equilibrium is disturbed by any factor, the…

Q: Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its…

A: A chemical reaction's equilibrium constant is the measure of the reaction quotient at chemical…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Question

100%

When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to
K (the equilibrium constant). If a stress is applied to the mixture that changes
the value of Q, then the system is no longer at equilibrium. To regain equilibrium,
the reaction will either proceed forward or in reverse until Q is equal to Konce
again. Alternatively, equilibrium can be disrupted by a change in temperature,
which changes the value of K. The result however is the same, and the reaction
will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's
principle summarizes this idea:
If a stress is applied to a reaction mixture at equilibrium, a net reaction occurs in
the direction that relieves the stress.

The following system is at equilibrium:X(s) + 3Y(g) = Z(g) Classify each of the following actions by whether it causes leftward shift, a rightward shift, or no shift in the direction of the net
reaction.
Decrease the volume
Leftward shift
Remove some X
Rightward shift
Increase the volume
No shift
Reset
Help
Add more X

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 250,(g)+O,(g) → 2So,(g) Suppose a mixture of SO,, O, and SO, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium to the right The pressure of O2 will to the left Some So, is added. The pressure of SO3 will ? (none) to the right The pressure of SO2 will ? Some SO3 is removed. to the left The pressure of O2 will (none) O O
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. 1.80 at 250 °C A 0.2950 mol sample of PCl, (g) is injected into an empty 4.75 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCl,] = M [PCI,] = M
A chemical engineer is studying the following reaction: HCN(aq)+NH,(aq) → CN (aq)+NH(aq) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.0. The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound concentration expected change in concentration vessel HCN 0.06 M O f increase OI decrease O (no change) NH, 0.22 M f increase OI decrease (no change) A CN 0.97 M increase I decrease (no change) NH, 1.23 M f increase OI decrease O (no change) HCN 0.53 M f increase OI decrease (no change) NH, 0.69 M f increase O I decrease (no change) В CN 0.50 M t increase OI decrease O (no change) NH, 0.76 M f increase Ot decrease (no change)…
Calculating an equilibrium constant from a partial equilibrium composition Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 500. mL flask with 3.3 atm of ammonia gas and 0.87 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.6 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = [] p ☐ x10 ☑ 00 18 Α
Steam reforming of methane ( CH, ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 2.0 L flask with 3.8 atm of methane gas and 2.0 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 3.0 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K, 0 x10 ?
-12. At a certain temperature, the equilibrium constant K for the following reaction is 6.08 x 10 : Br,(g) + OC1,(g) → BROCI(g) + BrCl(g) Use this information to complete the following table. Suppose a 43. L reaction vessel is filled with 1.7 mol of BrOCI and 1.7 mol of BrCl. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little Br, and OCI2. x10 There will be very little BrOCI and BrCl. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K =0 BROCI(g)+BrCl(g) Br,(9)+OCl,(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K =| 3 Br,(9)+30C1,(9) 3 BrOCl(g)+3BrCl(g)
Please don't provide handwritten solution .....
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 500. mL flask with 1.2 atm of sulfur dioxide gas and 4.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.60 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K, -0 x10 5
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) – PCI, (g) + Cl, (g) K. = 1.80 at 250 °C A 0.1997 mol sample of PCl, (g) is injected into an empty 2.40 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCl,] = M [PCl,] = M
Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 2 SO₂(g) + O₂(g) → 2 SO 3(g) The reaction is exothermic. Suppose a mixture of SO2, O₂ and SO3 has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation The temperature is lowered. change in composition The pressure of SO3 will The temperature is raised. The pressure of SO₂ will ? ? î ↑ shift in equilibrium O X to the right to the left (none) to the right to the left (none) S
Ammonia and oxygen react to form nitrogen and water, like this: 4NH3(g)+30₂(g) → 2N₂(g) + 6H₂O(g) Suppose a mixture of NH3, O₂, N₂ and H₂O has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation Some NH3 is removed. Some N₂ is added. change in composition The pressure of O₂ will The pressure of N₂ will The pressure of NH3 will The pressure of O₂ will ? ? ? ? O O C C shift in equilibrium O to the right Oto the left O (none) X O to the right O to the left O (none) 5 E C
Hydrogen and fluorine react to form hydrogen fluoride, like this: H,(g)+F2(g) → 2 HF (g) The reaction is exothermic. Suppose a mixture of H,, F, and HF has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. 圖 do perturbation change in composition shift in equilibrium O to the right The temperature is raised. The pressure of H2 will O to the left go up. (none) go down. not change. to the right The temperature is lowered. to the left The pressure of HF will O (none) Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center Accessibility DII 80 F10 FB F9 F6 F7 FS F4 esc F3 F1 @ # $ dele - 7 8. 2 3 4