In a galvanic cell, oxidation occurs at the anode.

In a galvanic cell, reduction occurs at the cathode.

Average rate = (change in concentration) / (time) = (0.5 - 0.1) / 20 = 0.02 M/min.

For the reaction A → B, the rate of disappearance of A is equal to the rate of formation of B, hence it is 0.1 mol/L·s. However, if stoichiometry is considered as 1:1, the rate of disappearance of A is also 0.1 mol/L·s.

For the reaction A → B, the rate of disappearance of A is equal to the rate of formation of B, thus it is 1.0 mol/L·s.

If the rate doubles when the concentration of A is doubled, the reaction is first order with respect to A.

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 position to the right to produce more products.

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

If ΔH is negative and ΔS is positive, ΔG will always be negative at all temperatures.

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.

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

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.