According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position 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, as the system tries to absorb the added heat.

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

Increasing the temperature of an exothermic reaction shifts the equilibrium to the left (towards the reactants), while for an endothermic reaction, it shifts to the right (towards the products).

At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction, which means the concentrations of reactants and products remain constant over time.

According to Le Chatelier's principle, if the concentration of products increases, the equilibrium will shift to the left to counteract the change.

According to Le Chatelier's principle, if the concentration of products increases, the equilibrium will shift to the left to counteract the change.

According to Le Chatelier's principle, if the concentration of products increases, the system will shift to the left, decreasing the rate of the forward reaction.

According to Le Chatelier's principle, increasing the concentration of products will shift the equilibrium position to the left to counteract the change.

According to Le Chatelier's principle, increasing the concentration of products will shift the equilibrium to the left to counteract the change.

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.

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

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

If the forward reaction is exothermic, the reverse reaction must be endothermic, as it absorbs heat.

In a rhombus, opposite angles are equal.

In a rhombus, the diagonals are unequal and bisect each other at right angles.

In a rhombus, the diagonals are perpendicular and they bisect the angles.

The side opposite to the 30-degree angle is half the hypotenuse, so it is 10/2 = 5 cm.

Opposite side = hypotenuse * sin(30°) = 10 * 1/2 = 5 cm.

In a right triangle, the sum of the angles is 180 degrees. Therefore, the other angle is 180 - 90 - 30 = 60 degrees.

In a 30-60-90 triangle, the sides opposite the 30 degrees and 60 degrees are in the ratio 1:√3.

In a 30-60-90 triangle, the sides opposite the 30 degrees and 60 degrees angles are in the ratio 1:√3.

In a right triangle, the sum of the angles is 180 degrees. If one angle is 45 degrees and the right angle is 90 degrees, the other angle must be 180 - (90 + 45) = 45 degrees.

In a right triangle, the sum of the angles is 180 degrees. Therefore, the other angle must be 180 - 90 - 30 = 60 degrees.

Using the Pythagorean theorem, b = √(c² - a²) = √(13² - 5²) = √(169 - 25) = √144 = 12.

In a right triangle, the sum of the angles is 180 degrees. If one angle is 30 degrees and the right angle is 90 degrees, the other angle must be 60 degrees.

In a right triangle, the sum of the angles is 180 degrees. Therefore, the other angle is 90 - 30 = 60 degrees.

In a right triangle, the sum of the angles is 180 degrees. Therefore, the other non-right angle must also be 45 degrees.

The sides opposite 30° and 60° are in the ratio 1:√3.

Using the Pythagorean theorem, b = √(c² - a²) = √(10² - 6²) = √(100 - 36) = √64 = 8.