Mass percentage = (mass of solute / mass of solution) × 100. Mass of solution = 10 g + 100 g = 110 g. Mass percentage = (10 g / 110 g) × 100 = 9.09%, approximately 10%.

Concentration = (10 g / 0.5 L) = 20 g/L.

Mass/volume % = (mass of solute / volume of solution) * 100 = (10 g / 500 mL) * 100 = 2%.

Concentration = mass / volume = 15 g / 300 mL = 0.05 g/mL.

Moles of glucose = 20 g / 180 g/mol = 0.111 M. Molarity = 0.111 moles / 1 L = 0.11 M.

Molality (m) = moles of solute / kg of solvent; assuming 1 L of water = 1 kg, m = 3 moles / 1 kg = 3 m

C1V1 = C2V2; (0.1 M)(50 mL) = C2(250 mL); C2 = 0.02 M.

Using M1V1 = M2V2, (3 M)(50 mL) = M2(200 mL) => M2 = (3 M × 50 mL) / 200 mL = 0.75 M.

According to Le Chatelier's principle, if a change is made to a system at equilibrium, the system will adjust to counteract that change. Increasing the concentration of a reactant will shift the equilibrium to the right, favoring the formation of products.

For a second-order reaction, if concentration is tripled, the rate increases by 3² = 9 times.

Increasing the concentration of Cu²⁺ increases the cell potential according to the Nernst equation.

pH = 3 means [H+] = 10^-3 M = 0.001 M.

For a weak acid, pH ≈ pKa for a 0.1 M solution, so pH ≈ 4.76.

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.