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

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

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.

The slowest step in a reaction mechanism is called the rate-determining step, as it controls the overall reaction rate.

The slowest step in a reaction mechanism is known as the rate-determining step.

According to the balanced equation 2H2 + O2 → 2H2O, 2 moles of H2 produce 2 moles of H2O.

At high temperatures, ΔG will be positive because the positive ΔH and negative ΔS will dominate the equation ΔG = ΔH - TΔS.

The mole ratio of A to C is 3:4 based on the coefficients in the balanced equation.

ΔG = ΔH - TΔS = -100 kJ - (298 K * 0.2 kJ/K) = -100 kJ - 59.6 kJ = -159.6 kJ.

Using the Arrhenius equation, Ea can be estimated to be around 40 kJ/mol.

The oxidizing agent is the species that gains electrons and is reduced.

In a reversible process, the change in entropy of the universe is zero, as the system and surroundings are in equilibrium.

In a reversible process, the change in Gibbs free energy (ΔG) is zero at equilibrium.

In a reversible process at equilibrium, the change in Gibbs free energy is zero.

Mole fraction of solute = moles of solute / (moles of solute + moles of solvent) = 1 / (1 + 9) = 0.1.

Mole fraction of A = moles of A / (moles of A + moles of B) = 3 / (3 + 1) = 0.75.

The addition of a non-volatile solute raises the boiling point of the solvent, a phenomenon known as boiling point elevation.

The presence of a non-volatile solute lowers the vapor pressure of the solvent compared to that of the pure solvent.

Using Raoult's Law, the vapor pressure of the solution is P_total = (0.6 * 100) + (0.4 * 50) = 60 + 20 = 80 mmHg.

The total vapor pressure of a solution is the sum of the partial vapor pressures of its components: 80 mmHg + 20 mmHg = 100 mmHg.

For a spontaneous process, the change in Gibbs free energy (ΔG) is negative.

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.

For equilibrium, the net force acting on the system must be zero.

The resultant force can be found using the Pythagorean theorem since the forces are perpendicular.