State the exothermic chemical reaction

Reference no: EM13161388

The exothermic chemical reaction CO(g) + H2O(g) CO2(g) + H2(g) has Kc = 0.034 at 25°C. We currently have a flask containing all the components listed in this equation at equilibrium at 25°C. Subsequently, we will either (1) add some H2 to the flask or (2) raise the temperature of the flask. What direction will the chemical equation shift for each of these separate actions, respectively, as the system re- approaches equilibrium? please explain! I'm confused about when temperature affects the K value, since it seems to have different things its determined by.

Reference no: EM13161388

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State the exothermic chemical reaction : The exothermic chemical reaction CO(g) + H2O(g) CO2(g) + H2(g) has Kc = 0.034 at 25°C. We currently have a flask containing all the components listed in this equation at equilibrium at 25°C. Subsequently, we will either (1) add some H2 to the flas..

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