The mole fraction of the solute is 1 - X_solvent = 1 - 0.8 = 0.2.

The mole fraction of the solvent is 1 - X_solute = 1 - 0.2 = 0.8.

Molarity = π / (RT) = 3.0 / (0.0821 * 298) = 0.12 M

Molarity = π / (RT) = 3.0 / (0.0821 * 298) = 0.12 M

The maximum number of electrons in a subshell is given by 2(2l + 1). For l = 2, it is 2(2*2 + 1) = 10.

For n=4, l can take values 0, 1, 2, or 3.

For n=4, l can take values from 0 to n-1, which are 0, 1, 2, and 3.

The discriminant must be less than zero: k^2 - 4*1*9 < 0 => k^2 < 36 => |k| < 6.

Using the Arrhenius equation, a rule of thumb states that for every 10°C increase in temperature, the rate doubles if Ea is around 40 kJ/mol.

For real and distinct roots, the discriminant must be positive: 3^2 - 4*1*k > 0 => 9 - 4k > 0 => k < 9.

Using Vieta's formulas, k = (-2)(-3) = 6.

Using Vieta's formulas, k = 2 * 4 = 8.

Ksp = [Ag+][Cl-] = s^2, thus s = sqrt(1.77 x 10^-10) = 1.77 x 10^-5 M.

According to Charles's Law, at constant pressure, the volume of a gas is directly proportional to its temperature.

As the temperature of a system increases, the kinetic energy of the particles increases, leading to greater disorder and thus an increase in entropy.

Using Raoult's Law, P_solution = X_solvent * P_pure_solvent; 60 mmHg = X_solvent * 80 mmHg; X_solvent = 60/80 = 0.75.

Using Raoult's Law, P_solution = X_solvent * P_solvent^0; 80 = X_solvent * 120; X_solvent = 80/120 = 0.67.

Using Raoult's Law, P_solution = X_A * P_A^0 = 0.6 * 100 mmHg = 60 mmHg.

According to Raoult's Law, P_solution = X_A * P_A^0 = 0.5 * 100 mmHg = 50 mmHg.

According to Raoult's Law, the vapor pressure of the solution is 0.5 * 100 mmHg = 50 mmHg.

Using Raoult's Law, the vapor pressure of the solution is P_solution = P_solvent * X_solvent = 120 * (1/(1+0.2)) = 120 * (1/1.2) = 100 mmHg.

Using Raoult's Law, P_solution = X_solvent * P_solvent^0 = 0.75 * 80 mmHg = 60 mmHg.

Using Raoult's law, the vapor pressure lowering is calculated considering the van 't Hoff factor for NaCl.

Subtracting 4 from both sides gives x = 6.

A negative ΔG indicates that the reaction is spontaneous.

A negative ΔG indicates that the reaction is spontaneous under the given conditions.

A negative ΔG indicates that the reaction is spontaneous.

If ΔG is positive, the reaction is non-spontaneous under the given conditions.

ΔG = ΔH - TΔS = 100 kJ - 298 K * 0.2 kJ/K = 100 kJ - 59.6 kJ = 40.4 kJ.

If ΔH is negative and ΔS is positive, ΔG will always be negative, indicating that the reaction is spontaneous at all temperatures.