ΔU = Q - W = 100 J - 40 J = 60 J.

If the internal energy of a closed system increases, it indicates that work is done on the system.

If the internal energy increases in a closed system, the enthalpy also increases, as ΔH = ΔU + PΔV.

According to Boyle's Law, if the volume is halved, the pressure will double (P1V1 = P2V2).

According to Boyle's Law, if the volume is halved, the pressure will double (P1V1 = P2V2).

According to Boyle's Law, decreasing the volume of a gas at constant temperature increases the pressure.

E = E° - (0.059/n)log([Ag⁺]1/[Ag⁺]2); E = 0 - (0.059/1)log(10) = 0.059 V.

E = (0.059 V/n) * log([Cathode]/[Anode]) = (0.059 V/2) * log(10) = 0.059 V.

E = (0.059 V/n) * log([Cathode]/[Anode]) = (0.059 V/2) * log(1/0.1) = 0.059 V * 1 = 0.059 V.

In a concentration cell, the cell potential is dependent on the concentration differences of the reactants.

In a concentration cell, the cell potential is generated due to differences in ion concentrations.

For a constant pressure process, the work done by the system is related to the change in enthalpy by the equation ΔH = Q + PΔV, where Q is the heat added.

The work done in a constant pressure process is calculated using W = PΔV, where P is pressure and ΔV is the change in volume.

The work done by the system at constant pressure is given by W = PΔV, where P is pressure and ΔV is the change in volume.

The salt bridge maintains charge neutrality by allowing ions to flow between the two half-cells.

In a Daniell cell, the zinc electrode acts as the anode where oxidation occurs, releasing electrons.

In a Daniell cell, Cu²⁺ is reduced to Cu at the cathode.

For a first-order reaction, the half-life (t1/2) is given by t1/2 = 0.693/k. Rearranging gives k = 0.693/t1/2 = 0.693/10 min = 0.0693 min^-1.

For a first-order reaction, the concentration after n half-lives is given by [A] = [A]0 * (1/2)^n. After 30 minutes (3 half-lives), [A] = 1 M * (1/2)^3 = 0.125 M.

For a first-order reaction, the half-life is independent of the initial concentration. Therefore, it remains 10 minutes.

For a first-order reaction, the half-life is independent of concentration. Therefore, the half-life remains 10 minutes.

For first-order reactions, the half-life is independent of concentration but depends on the rate constant, which increases with temperature. Typically, the half-life will decrease, but the exact value requires the Arrhenius equation.

The half-life of a first-order reaction is constant and does not depend on the concentration; it remains 10 minutes.

The cathode reaction involves the reduction of Cu²⁺ to Cu: Cu²⁺ + 2e⁻ → Cu.

The external circuit provides a path for electrons to flow from the anode to the cathode.

In a galvanic cell, oxidation occurs at the anode, where the reducing agent loses electrons.

In a galvanic cell, oxidation occurs at the anode, where electrons are released.

A triple bond consists of 1 sigma bond and 2 pi bonds.

The line between the solid and liquid phases in a phase diagram represents the melting point, where solid and liquid coexist.

For a 1:1 stoichiometry, the rate of disappearance of A is equal to the rate of formation of B. Therefore, it is 0.5 M/s, but since A is disappearing, it is 1.0 M/s.