Modern Chemistry Chapter 18 Section 1 Review Answers

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Chemical Equilibrium Chapter 18 Modern Chemistry PowerPoint Presentation

Chemic Equilibrium Chapter 18 Modern Chemistry

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Chemical Equilibrium Chapter 18 Modern Chemical science

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1. ChemicalEquilibriumChapter 18 Modernistic Chemical science Sections i & 2 The Nature of Chemical Equilibrium Shifting Equilibrium Affiliate 18 Section 1 Chemic Equilibrium p. 589-597

2. Section 18.1 The Nature of Chemical Equilibrium Chapter eighteen Section 1 ChemicaL Equilibrium p. 589-597

3. Vocabulary • Reversible Reaction • Chemical Equilibrium • Equilibrium Expression • Equilibrium Constant • LeChatelier'due south Principle Insert Holt Disc 2 Affiliate 18 Department 1 Chemic Equilibrium p. 589-597

4. Reversible Reactions Insert Holt Disc 2 Insert Glencoe Disc i Chapter 18 Section 1 Chemic Equilibrium p. 589-597

5. Reversible Reactions • Products tin react to re-course the reactants. • Must occur in a "closed" arrangement • 2HgO(s) 2Hg(fifty) + O2(g) • 2Hg(l) + O2(g) 2HgO(s) • Both of these reactions occur simultaneously • 2HgO(s) 2Hg(l) + O2(g) Chapter 18 Section ane ChemicaL Equilibrium p. 589-597

6. Chemical Equilibrium • Charge per unit of its forward reaction equals the rate of its reverse reaction …. • and the concentrations of its products and reactants remain unchanged • Eventually all reversible reactions will reach eq. if the system is closed and atmospheric condition don't change. • Eq. is dynamic – always in motion. Chapter eighteen Department ane Chemic Equilibrium p. 589-597

7. Reaction Rate vs time p. 591 Chapter 18 Section i Chemical Equilibrium p. 589-597

8. Equilibrium Sit-in Chapter 18 Department 1 ChemicaL Equilibrium p. 589-597

9. Reaction Rate vs. Fourth dimension p. 591 Rateforward = Ratereverse Affiliate 18 Section ane Chemical Equilibrium p. 589-597

10. What is "favored" at Eq? • At equilibrium equal rates! reactants are favored neither is favored products are favored R P Chapter 18 Section 1 Chemical Equilibrium p. 589-597

11. Equilibrium Expression [ ] = concentration in mol/Fifty • northward A + m B x C + y D • Dependant on temperature • Independent of initial concentrations [C]ten [D]y products Keq = = [A]n[B]m reactants 10, y, n, chiliad = coefficients Chapter 18 Section 1 ChemicaL Equilibrium p. 589-597

12. Equilibrium Constant PRODUCTS • If Keq is big (>i) so products are favored at eq. • If Keq is small (<1) then reactants are favored at eq. Keq = REACTANTS PRODUCTS Keq = REACTANTS Pure liquids and solid are omitted. Chapter 18 Department 1 Chemic Equilibrium p. 589-597

13. Equilibrium Constants Tabular array Chapter 18 Department 1 ChemicaL Equilibrium p. 589-597

14. Sample Trouble p. 594 • An equilibrium mixture of N2, O2 , and NO gases at 1500 K is determined to consist of six.4x10–3 mol/Fifty of N2, one.7x10–3 mol/Fifty of O2, and 1.1x10–five mol/L of NO. What is the equilibrium constant for the system at this temperature? Keq = i.1 x ten−5 Chapter 18 Department 1 Chemical Equilibrium p. 589-597

15. Practice Issues p. 595 #i • At equilibrium a mixture of N2, H2, and NH3 gas at 500°C is determined to consist of 0.602 mol/L of N2, 0.420 mol/50 of H2, and 0.113 mol/Fifty of NH3.What is the equilibrium constant for the reaction N2(one thousand) + 3H2(one thousand) 2NH3(g) at this temperature? 0.286 Chapter xviii Section 1 Chemic Equilibrium p. 589-597

16. Do Problems p. 595 #two • The reaction AB2C(thou) B2(g) + AC(g) reached equilibrium at 900 K in a five.00 L vessel. At equilibrium 0.084 mol of AB2C, 0.035 mol of B2, and 0.059 mol of AC were detected. What is the equilibrium abiding at this temperature for this system? (Don't forget to convert amounts to concentrations.) 4.ix x 10−3 Chapter xviii Section one Chemical Equilibrium p. 589-597

17. Practice Problems p. 595 #iii • A reaction between gaseous sulfur dioxide and oxygen gas to produce gaseous sulfur trioxide takes identify at 600°C.At that temperature, the concentration of SO2 is found to be 1.fifty mol/50, the concentration of O2 is 1.25 mol/L, and the concentration of SO3 is 3.fifty mol/Fifty. Using the balanced chemical equation, calculate the equilibrium constant for this arrangement. 4.36 Chapter xviii Section one ChemicaL Equilibrium p. 589-597

18. Equilibrium Concentrationsand Keq values p. 593 Chapter 18 Department one ChemicaL Equilibrium p. 589-597

19. Eq. Concentration Problem • For the decomposition reaction of ammonia, 0.75 M of ammonia are added to an empty 1 50 flask. When the reversible reaction has achieved equilibrium the concentration of nitrogen in the flask is 0.fifteen M. Find the equilibrium concentrations of hydrogen and ammonia. Too find the Keq. Affiliate 18 Department 1 ChemicaL Equilibrium p. 589-597

20. Determining Eq. Concentrations N2 (g)+3 H2 (g) 2NH3(g) 1/3 = 0.15/x 10 = 0.45M 0 M 0 Thousand 0.75 M +0.15 M +0.45 M 0.15 M 0.45 Thousand Chapter 18 Department ane ChemicaL Equilibrium p. 589-597

21. Determining Eq. Concentrations N2 (yard)+3 H2 (grand) 2NH3(chiliad) 1/2 = 0.15/x 10 = 0.30M 0 Chiliad 0 M 0.75 M +0.15 Thou +0.45 M -0.xxx Chiliad 0.15 M 0.45 One thousand 0.45 M If this side is + then the other side is -. Chapter 18 Section one Chemical Equilibrium p. 589-597

22. Eq. Concentration Problem • For the synthesis reaction of hydrogen and iodine, 0.20M of hydrogen and 0.30M of iodine are added to an empty one L flask. When the reversible reaction has accomplished equilibrium the concentration of hydrogen in the flask is 0.10 G. Find the equilibrium concentrations of iodine and hydrogen iodide. Also detect the Keq. Chapter 18 Section 1 Chemic Equilibrium p. 589-597

23. Determining Eq. Concentrations H2 (g) + I2 (g)  2HI(thou) 1/1 = 0.10/10 x = 0.10M 0.20 M 0.xxx M 0 Thou -0.10 Yard -0.ten K 0.10 M 0.20 One thousand Chapter 18 Department 1 ChemicaL Equilibrium p. 589-597

24. Determining Eq. Concentrations H2 (g) + I2 (g)  2HI(one thousand) 1/two = 0.x/ten x = 0.20M 0.twenty M 0.30 K 0 Thousand -0.ten Thou -0.10 M +0.20 M 0.x M 0.twenty M 0.xx One thousand If this side is - then the other side is +. Affiliate 18 Section 1 Chemical Equilibrium p. 589-597

25. Eq Concentration Problem • A 0.20 G solution of HC2H3O2 is five.0% ionized. Detect the equilibrium concentrations of H+, C2H3O21- and HC2H3O2, besides observe the Keq. answer Chapter eighteen Section 1 Chemic Equilibrium p. 589-597

26. Eq Conc. & Keq Issues • At a specific temperature and pressure, 1.2 moles of hydrogen, 0.twoscore moles of nitrogen and 1.iii moles of ammonia are put into a closed one liter flask. When allowed to reach equilibrium the amount of ammonia is ane.6 moles. Detect the Keq for this arrangement. • N2(g) + 3H2(g) 2NH3(g) respond Affiliate eighteen Section 1 Chemical Equilibrium p. 589-597

27. Eq Conc. & Keq Bug • When .56 moles of SO3 is placed in a liter container, some of it decomposes. The equilibrium concentrations of SO2 is 0.42 moles / liter. Calculate the equilibrium concentration of O2 and SO3 and the Keq. O2 = 0.21 One thousand SO3 = 0.14 Thou Keq = .53 Chapter 18 Section 1 Chemical Equilibrium p. 589-597

28. Ch 18 Sec one Homework Page 595 # 1-nine Chapter xviii Section 1 ChemicaL Equilibrium p. 589-597

29. Ch 18 Sec one Homework Equilibrium Concentrations and Keq Worksheet Affiliate 18 Section one Chemical Equilibrium p. 589-597

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