Consider the reaction A(g) + B(g) C(g) + D(g). You have the gases A, B, C, and D at equilibrium. Upon adding gas A, the value of K: increases, because by adding A more products are made, increasing the product to reactant ratio decreases, because A is a reactant so the product to reactant ratio decreases does not change, because A does not figure into the product to reactant ratio does not change, as long as the temperature is constant depends on whether the reaction is endothermic or exothermic
Consider the reaction A(g) + B(g) C(g) + D(g). You have the gases A, B, C, and D at equilibrium. Upon adding gas A, the value of K: increases, because by adding A more products are made, increasing the product to reactant ratio decreases, because A is a reactant so the product to reactant ratio decreases does not change, because A does not figure into the product to reactant ratio does not change, as long as the temperature is constant depends on whether the reaction is endothermic or exothermic
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Consider the reaction A(g) + B(g) C(g) + D(g). You have the gases A, B, C, and D at equilibrium. Upon adding gas A, the value of K:
increases, because by adding A more products are made, increasing the product to reactant ratio
decreases, because A is a reactant so the product to reactant ratio decreases
does not change, because A does not figure into the product to reactant ratio
does not change, as long as the temperature is constant
depends on whether the reaction is endothermic or exothermic
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