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Unformatted text preview: · If: Qc < K c ­ Reaction will go to the r ight ( · If: Qc = Kc ­ Reaction mixture is at equilibrium ( ) ) Examples: The fo llowing reaction has an equilibrium constant , Kc, equal to 3.59 at 900 °C, and the fo llo wing co mposit ion of react ion mixture: CH4 (g) + 2 H2S (g) ¾¾ ® ¬¾ ¾ 1.26 M 1.32 M (a) Is the reaction mixture at equilibrium? CS2 (g) + 4 H2 (g) 1.43 M 1.12 M [H 2 ]4 [CS2 ] (1.12 M) 4 (1.43 M) Qc = = = 1.02 2 [CH 4 ][H 2 S]2 (1.26 M)(1.32 M) Qc = 1.02 Kc = 3.59 Qc ¹ Kc Not at equilibrium (b) If not at equilibrium, in which direct ion will the reaction go to reach equilibrium? Qc < K c Ø React ion will go to the right Ø Forward reaction is favored Ø Formation of products is favored 16 Chemistry 102 Chapter 14 CALCULATING EQUILIBRIUM CONCENTRATIONS · We can use equilibrium constant to calculate the equilibrium concentration of all the substances in the mixture. Some o f the variations that these problems occur are shown in the examples below: Example 1: Nitric oxide, NO, is formed in automobile exhaust by the reaction of...
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