For the reaction given, the value of the equilibrium of the constant at 400 K is 7.0. Br2(g)+ Cl2(g)=2BrCl(g)
Does the:
Reaction proceed to the left?
Reaction proceed to the right?
Partial pressure represent a system in an equation?
Write the K expression. Now, to have K 7.0 (greater than 1.0), must products or reactants be greater or less?
The reaction is favoring the products. In other words when you have a reaction whose number is 0 you are at a perfect equilibrium, when you have some number smaller than that you have a greater number of reactants than products. When you are above that you a greater number of products than compared to reactants. How do I know this? Kc= products/reactants
To determine the direction in which the given reaction proceeds (left or right), we need to compare the Q (reaction quotient) with the K (equilibrium constant).
The reaction quotient (Q) is calculated in the same way as the equilibrium constant (K), but it is calculated using the partial pressures of the reactants and products at a given point in time, rather than at equilibrium.
If Q < K, it means that at that particular point in time, the concentrations of reactants are lower and/or the concentrations of products are higher than they are at equilibrium. In this case, the reaction will proceed in the forward direction (to the right), to reach equilibrium.
If Q = K, it means that at that particular point in time, the concentrations of reactants and products are already in the same ratio as they are at equilibrium. In this case, the reaction is already at equilibrium, and there will be no net change in concentrations of reactants and products.
If Q > K, it means that at that particular point in time, the concentrations of reactants are higher and/or concentrations of products are lower than they are at equilibrium. In this case, the reaction will proceed in the reverse direction (to the left), to reach equilibrium.
Since the value of the equilibrium constant is given as 7.0, we can compare this value with Q to determine the direction of the reaction. If Q < K, the reaction will proceed to the right (forward direction), if Q > K, the reaction will proceed to the left (reverse direction), and if Q = K, the reaction is at equilibrium.
Regarding your second question, partial pressure does represent the system in an equation in the context of gaseous reactions. In the given reaction, the reactants and products are gases (Br2, Cl2, and BrCl), and their concentrations are represented by their partial pressures. The reaction quotient (Q) and the equilibrium constant (K) are calculated using the partial pressures of these gases.