For exothermic reactions, increasing the temperature shifts the equilibrium to the left, thus decreasing the equilibrium constant.

Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas. In this case, the right side has 2 moles of NH3 compared to 4 moles of reactants.

According to Le Chatelier's principle, decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the right side (2 moles of NH3).

The equilibrium constant Kp is expressed as Kp = (P_B^2 * P_C) / (P_A^3).

According to Le Chatelier's principle, increasing the concentration of a reactant will shift the equilibrium to the right.

Strong acid and strong base neutralize each other, resulting in a neutral solution with pH = 7.

Using the formula Ka = [H+]^2 / [HA], where [H+] = 10^(-4) M and [HA] = 0.1 M, we find Ka = (10^-4)^2 / 0.1 = 1 x 10^-5.

HCl and NaOH neutralize each other, resulting in a neutral solution with pH = 7.

In this case, the reaction force at each support is half the load applied at the center.

The horizontal component is calculated as 10 N * cos(30°) = 8.66 N.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.

The equilibrium constant for the reverse reaction is the reciprocal of the forward reaction, so Kc' = 1/Kc = 0.1.

A Kc value greater than 1 indicates that the products are favored at equilibrium.

A Kc value less than 1 indicates that at equilibrium, the concentration of reactants is greater than that of products, thus reactants are favored.

According to Le Chatelier's principle, increasing the temperature of an exothermic reaction shifts the equilibrium position to the left, favoring the reactants.

Increasing the pressure will shift the equilibrium position to the side with fewer moles of gas.

Increasing the pressure will shift the equilibrium to the side with fewer moles of gas, which in this case is the right side.

Decreasing the volume increases the pressure, and the equilibrium will shift to the side with fewer moles of gas to counteract the change.

Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the left side.

In a dynamic equilibrium, the rates of the forward and reverse reactions are equal, but the concentrations of reactants and products may not be equal.

According to Le Chatelier's principle, decreasing the concentration of a reactant will shift the equilibrium to the left to produce more reactants.

Decreasing the concentration of products will shift the equilibrium to the right to produce more products, according to Le Chatelier's principle.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium to the right to form more products.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right to produce more products.

For an exothermic reaction, decreasing the temperature shifts the equilibrium to the right, favoring the formation of products.

For an exothermic reaction, increasing the temperature shifts the equilibrium position to the left, favoring the reactants.

For an endothermic reaction, increasing temperature shifts the equilibrium to the right, increasing Kc.

Using the formula for weak bases, pH = 14 - pKb = 14 - (14 - 4.75) = 5.75.

If the sum of clockwise moments equals the sum of counterclockwise moments, the object is in equilibrium.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right to favor the formation of products.