In a Daniell cell, Zinc acts as the anode.

Using the first-order rate equation, k = (ln[A₀] - ln[A]) / t. Here, k = (ln(0.8) - ln(0.2)) / 20 = 0.0347 min⁻¹.

t₁/₂ = 0.693 / k = 0.693 / 0.03 = 23.1 min.

The cathode reaction must be a reduction reaction, and Cu²⁺ + 2e⁻ → Cu is a common cathode reaction.

The cathode reaction is O₂ + 4e⁻ + 4H⁺ → 2H₂O.

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.

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, increasing the concentration of reactants will shift the equilibrium position to the right to favor 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.

Zinc (Zn) is oxidized to Zn2+, so its oxidation state is +2.

Iron (Fe) is oxidized as it loses electrons to form FeCl3.

Fe2O3 is reduced to Fe, as it gains electrons during the reaction.