Concept explainers
(a)
Interpretation:
The direction in which the equilibrium for the given reaction will shift with an increase in the volume of the container is to be predicted.
Concept Introduction:
Le-Chatelier principle states that the when a dynamic equilibrium is subjected to a change, the equilibrium moves in a direction so as to counteract that change. If the volume of the container increases, the pressure of the container decreases. The equilibrium will shift in the direction in order to decrease the pressure and vice versa.
(b)
Interpretation:
The direction in which the equilibrium for the given reaction will shift with an increase in the volume of the container is to be predicted.
Concept Introduction:
Le-Chatelier principle states that the when a dynamic equilibrium is subjected to a change, the equilibrium moves in a direction so as to counteract that change. If the volume of the container increases, the pressure of the container decreases. The equilibrium will shift in the direction in order to decrease the pressure and vice versa.
(c)
Interpretation:
The direction in which the equilibrium for the given reaction will shift with an increase in the volume of the container is to be predicted.
Concept Introduction:
Le-Chatelier principle states that the when a dynamic equilibrium is subjected to a change, the equilibrium moves in a direction so as to counteract that change. If the volume of the container increases, the pressure of the container decreases. The equilibrium will shift in the direction in order to decrease the pressure and vice versa.
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Chapter 17 Solutions
Introductory Chemistry: A Foundation
- lum constant Suppose a 500. mL flask is filled with 0.30 mol of I, and 1.9 mol of HI. The following reaction becomes possible: H,(g) + I,(g) = 2 HI(g) The equilibrium constant K for this reaction is 5.08 at the temperature of the flask. Calculate the equilibrium molarity of I,. Round your answer to two decimal places. M Check 2021 McG N Explgationarrow_forwardHelp 1arrow_forwardChemistry practice questionarrow_forward
- Suppose a 250. mL flask is filled with 0.70 mol of N, and 0.50 mol of NO. The following reaction becomes possible: N,(8) + 0,(g) – 2 N0(3) The equilibrium constant K for this reaction is 8.44 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Explanation Check 2021 McGraw-Hill Education. All Rights Reserved acerarrow_forward? QUESTION Bromine and water react to form hydrogen bromide and oxygen, like this: 2 Br,(g) + 2 H,0(g) 4 HBr(g) +02(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of bromine, water, hydrogen bromide, and oxygen has the following composition: compound concentration at equilibrium Br, 0.81 M H,0 0.79M HBr 1.4M O2 1.1M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac), A v BIUS Paragraph Arial 10pt Save All Answer Click Save and Submit to save and submit. Click Save All Answers to save all answers.arrow_forwardQuestion 15 Nitrogen gas (N2) and oxygen gas (O2) are Sealed in an empty container with a volume of 2 dm°, After a while the following equilibrium is reached: N2(g) + O2(g) = 2NO(g) The Kc value of this reaction is 4,3 x 101 at 25 C. 15.1 What information does this Ke value provide about the amount NO(g) in the equilibrium mixture at 25°C? 15.2 The flask is heated and the system reaches a new equilibrium at 2 500°C. It is determined. that at this temperature there are 1,8 mol O2(g) and 0,4 mol NO(g) and that the Ko value is 0,013. 15.2.1 Calculate the concentration of N2 at the new equilibrium. 15.2.2 How many mcles of N2 were initially placed in the container? 15.2.3 What type of reaction is the forward reaction, endothermic or exotihermic? QUESTIONSarrow_forward
- Problem 7 For the chemical reaction 2A + B 2 C, suppose that the equilibrium constant is determined to be Keg=111 at a temperature of 310 K. a) Calculate the value of AGrxn at this temperature. b) Consider a case where all concentrations are equal, i.e., [A]=[B]=[C]=x. What concentration x would correspond to the reaction being in equilibrium at 310K?arrow_forwardissue 13Balance the reaction below and write the expression for the equilibrium constant. NO(g) + Cl2(g) ⇌ NOCl(g)I found as a balanced equation: 2NO(g) + Cl2(g) ⇌ 2NOCl(g) and as Kc= 2.5 x 103.Is it correct ?arrow_forward2) Answer this with complete solution, and give what’s required and the given.arrow_forward
- Please correct answer and don't use hend raitingarrow_forwardCheck Your Understanding Nitrogen oxides in the atmosphere may acidify rainwater. Write the equilibrium expression for the following reaction in which gaseous nitrous acid forms in the atmosphere: NO(g) + NO2(g) + H2O(g) 2 2 HNO2(g) Answer [HNO2J? K = NO][NO2][H2 O]arrow_forwardFor the following reaction 3O₂(g) ⇌ 2O₃(g) Kc = 2.10 × 10⁻⁷ at a certain temperature. If [O₂] = 0.0365 M when at equilibrium, what is the equilibrium O₃ concentration? Answer ___ Marrow_forward
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