Using the Arrhenius equation, if the rate doubles for a 10°C increase, Ea is approximately 40 kJ/mol.

The order of the reaction is third because the rate is proportional to the concentration raised to the power of 3.

The reaction is second-order because the rate depends on the square of the concentration of A.

Molar mass of H2SO4 = 2*1 + 32 + 4*16 = 98 g/mol. Mass = 0.25 moles x 98 g/mol = 24.5 g.

A buffer solution typically consists of a weak acid and its conjugate base (salt), which helps to resist changes in pH when small amounts of acid or base are added.

A buffer solution is made from a weak acid and its conjugate base (salt), which helps maintain pH.

The efficiency of a Carnot engine is given by η = 1 - T2/T1.

The efficiency of a Carnot engine is determined by the temperatures of the hot and cold reservoirs, given by the formula η = 1 - (T_c/T_h).

According to the First Law of Thermodynamics, ΔU = Q - W. Here, ΔU = 100 J - 40 J = 60 J.

Using the Nernst equation, E = (0.0591/n) log([C1/C2]), where n=1.

In a cyclic process, the net work done is equal to the net heat added to the system, as the internal energy returns to its initial state.

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.

In a first-order reaction, the half-life is constant, which indicates that the rate constant remains constant.

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 system will shift to the left, decreasing the rate of the forward reaction.

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 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.

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.