The cathode reaction must be a reduction; Ag⁺ + e⁻ → Ag is the anode reaction.

The cathode reaction is Cu²⁺ + 2e⁻ → Cu.

Efficiency (η) = Work done / Input heat = 300 J / 500 J = 0.6 or 60%.

Average rate = Δ[A]/Δt = (0.8 - 0.4) / 20 = 0.02 M/min.

For a first-order reaction, if [A] is halved, the rate also halves.

If the rate decreases to one-fourth when concentration is halved, the reaction is second-order.

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.

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, 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 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.

For a second-order reaction, t₁/₂ = 1 / (k[A₀]) = 1 / (0.05 * 0.1) = 200 s.

For a zero-order reaction, the rate is constant and does not depend on the concentration of reactants. The unit of the rate constant (k) is mol/L·s.

In a zero-order reaction, the rate is constant and does not depend on the concentration of the reactants.

In an adiabatic process, the relationship is given by PV^n = constant, where n is the heat capacity ratio.

In an adiabatic process, there is no heat exchange with the surroundings, meaning no heat is absorbed or released.

In an adiabatic process, there is no heat exchange, so the internal energy remains constant for an ideal gas.

For an ideal gas, the internal energy depends only on temperature. Since the temperature remains constant in an isothermal process, the internal energy also remains constant.

In an isothermal process, the temperature of the system remains constant.

1 mole of Cu²⁺ deposits 63.5 g of copper.

Using the formula: moles = (current × time) / (n × F), where n=1 for electrons and F=96500 C/mol.

In electrolysis, oxidation occurs at the anode.

In electrolysis, oxidation occurs at the anode.

Chlorine gas is produced at the anode during the electrolysis of NaCl solution.