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(a)
Interpretation:
Shift of equilibrium with increase in temperature in below reaction has to be determined.
Concept Introduction:
Le Chatelier’s principle states that changes at equilibrium in system respond to reduce the changes and bring back the system to restore its equilibrium under new conditions. According to this principle with increase in temperature reaction rate rises due to rise in kinetic energy. In case of endothermic reaction that is when energy is absorbed then the reaction moves in forward direction. In case of exothermic reaction that is when energy is released then reaction moves in backward direction.
(b)
Interpretation:
Shift of equilibrium with increase in temperature in below reaction has to be determined.
Concept Introduction:
Refer to part (a).
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Chapter 16 Solutions
FOUND.OF COLLEGE CHEMISTRY
- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forwardDescribe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.arrow_forwardWrite an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a productarrow_forward
- Be sure to answer all parts. Given the value of the equilibrium constant (K) for equation (a), calculate the equilibrium constant for equation (b). 2 (a) O2(g) S,03(g) K = 8.58 × 10-9 %3D х 10 (Enter your answer in scientific notation.) (b) 302(g) 5 203(g)arrow_forwardThe equilibrium constant, Kc, for the following reaction is 6.54 × 10-³ at 298 K. -3 2NOBr(g) 2NO(g) + Br₂(g) Calculate Ke at this temperature for the following reaction: с NO(g) + 1/2Br2(g) → NOBr(g) Kc =arrow_forwardConsider the equilibrium C(s) + H2O(g) CO(g) + H2(g), ΔH = 2296 J. The concentration of carbon will not change if gaseous water is added to the system. True or False?arrow_forward
- 2) 2.44 mol of gaseous hydrogen bromide is added to an empty 3.16 L container. When values are no longer changing, at 62.5 °C, 0.55 mol hydrogen gas is collected. Using the provided skeletal equation, determine the value of the equilibrium constant, at 62.5 °C, to 2 decimal Br2(8) HBr f Bre) Brie) + H, 2(8) [K5] places:arrow_forward2. Given the reaction: N2(g) + 3H2 (g) = 2NH3 (g) If Kc for this reaction is 4.5 x 10-4 at 400 K, what is the equilibrium constant KR at the same temperature?arrow_forwardCalculate the value of the equilibrium constant (Keg) for the following reaction: 2 CO (g) + 6 H2 (g) → 2 CH4 (g) + 2 H2O (g) The following two equilibrium reactions should be helpful in determining this value: CO (g) + 2 H2S (g) <→ CS2 (g) + H2O (g) + H2 (g) ½ CH4 (g) + H2S (g) <→ ½ CS2 (g) + 2 H2 (g) Reaction 1: K1 = 1.3 x 105 Reaction 2: K2 = 180 (A) 2.3 x 107 (B) 1.9 x108 (C) (D) 16.1 722 (E) 1.5 x 10-8arrow_forward
- The equilibrium constant for the reaction2 NO(g) + Br2(g) ⇌ 2 NOBr(g)is Kc = 1.3 x 10-2 at 1000 K. (a) At this temperature doesthe equilibrium favor NO and Br2, or does it favor NOBr?(b) Calculate Kc for 2 NOBr(g)⇌ 2 NO(g) + Br2(g).(c) Calculate Kc for NOBr(g)⇌ NO(g) + 1/2 Br2(g).arrow_forward٧arrow_forwardWhat's the equilibrium expression for the following reaction:arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
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