ΔG = ΔH - TΔS = 200 kJ - 400 K * 0.5 kJ/K = 200 kJ - 200 kJ = 0 kJ.

The rate of disappearance of A is equal to the rate of formation of B, multiplied by the stoichiometric coefficients. Here, it is 1.0 mol/L/s.

If doubling the concentration of A doubles the rate, the reaction is first order with respect to A.

The correct relationship at constant temperature and pressure is ΔG = ΔH - TΔS.

According to Le Chatelier's principle, if the concentration of products increases, the equilibrium will shift to the left.

If ΔG° is negative, the equilibrium constant K is greater than 1.

A positive ΔG° indicates that the reaction is non-spontaneous in the forward direction, thus spontaneous in the reverse.

A positive ΔG° indicates that the reaction is non-spontaneous in the forward direction under standard conditions.

A positive ΔG° indicates that the reaction is non-spontaneous in the forward direction.

To find the temperature at which the reaction becomes spontaneous, set ΔG = 0: 0 = ΔH - TΔS. Thus, T = ΔH/ΔS = (100,000 J)/(200 J/K) = 500 K.

To find the temperature at which the reaction becomes spontaneous, set ΔG = 0: 0 = ΔH - TΔS, thus T = ΔH/ΔS = 100,000 J / 200 J/K = 500 K.

To find the temperature at which the reaction becomes spontaneous, set ΔG = 0: 0 = ΔH - TΔS, thus T = ΔH/ΔS = (50,000 J/mol) / (100 J/mol·K) = 500 K.

For a reversible process, the change in entropy is given by ΔS = Q/T, where Q is the heat exchanged and T is the temperature.

For a reversible process, the change in entropy (ΔS) is given by ΔS = Q/T, where Q is the heat absorbed and T is the temperature.

The change in entropy (ΔS) for a reversible process is given by ΔS = Q/T, where Q is the heat absorbed and T is the temperature.

For a reversible process, the change in entropy of the universe is zero, as the system and surroundings are in equilibrium.

The efficiency of a Carnot engine is given by η = 1 - (T2/T1), where T1 is the temperature of the hot reservoir and T2 is the temperature of the cold reservoir.

For a solution to obey Raoult's Law, the interactions between solute and solvent must be similar to those in the pure components.

For a spontaneous process, the total entropy change of the universe (system + surroundings) must be positive.

The relationship is given by ΔG = ΔH - TΔS, where ΔG must be negative for a spontaneous process.

The correct relationship is ΔG = ΔH - TΔS, where ΔG must be negative for a spontaneous process.

For a process to be spontaneous, the change in Gibbs free energy (ΔG) must be negative.

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

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

For d orbitals, the azimuthal quantum number l = 2.

For l=2 (d orbital), m_l can take values from -l to +l, which are -2, -1, 0, 1, 2.

For a p orbital, l=1, so m_l can take values -1, 0, +1.

For a p orbital (l=1), m_l can take values -1, 0, +1.

For l=2 (d orbital), m_l can take values from -2 to +2, which are -2, -1, 0, 1, 2.

According to Raoult's Law, the vapor pressure of the solution is 0.75 * 100 mmHg = 75 mmHg.