Learning Goal: To understand how reactions at equilibrium respond to changes in

Question

Learning Goal: To understand how reactions at equilibrium respond to changes in conditions, including volume changes and addition of reactants or products. Equilibrium equations can be used to determine what will happen to a system at equilibrium if certain conditions are changed (e.g., the addition of a reactant or product or-in the case of gaseous reactions-a volume change). For example, given the reaction 1/8S8(s) + O2(g) SO2(g) what will happen to the system if more SO2 (g) is added so that the concentration of SO2 (g) is doubled? The equilibrium equation is given by K = [SO2]/[O2] Equilibrium equations do not include expressions for any pure solids or liquids that may be involved in the reaction. This is because at any given temperature their concentration is constant, and these values are by convention included in the value of the equilibrium constant. Since the value of K remains constant for the reaction at any given temperature, if the value of [SO2] is doubled, then the value of [O2] must also double to return the system to equilibrium. For the decomposition of A to B and C, A (s) B(g) + C(g) how will the reaction respond to each of the following changes at equilibrium? Drag the appropriate items to their respective bins. For the reaction of A and B forming C, A(g) + B(s) 2C(g) how will the reaction respond to each of the following changes at equilibrium? Drag the appropriate items to their respective bins.

Explanation / Answer

We Know that :     The given Reaction is :            A( g ) + B ( s ) <-------> 2 C ( g )           halvethe concentration of C - Equilibrium shifts to Rightwards           halvethe concentration of A = Equilibrium shifts toLeftwards           double the concentration of A and C = Equilibriumshifts to Leftwards as the concentration of product issquared             double the concentration A = Equilibrium shifts to Rightwards               quadraple the concentration of B = No shift.            A( s )   <--------> B (g ) + C ( g )           For theabove Reaction their will be no shift in the equilibrium as theequilibrium constant is independent of the          concentration of A as A is solid in nature.

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