The ideal gas constant R is 0.0821 L·atm/(K·mol).

R can have different values depending on the units used, including 0.0821 L·atm/(K·mol), 8.314 J/(K·mol), and 62.36 L·mmHg/(K·mol).

Kc = ([C][D]) / ([A][B]) = (0.3 * 0.4) / (0.1 * 0.2) = 2.0

Kc = [C]/([A][B]) = 0.3/(0.1*0.2) = 1.5

Kc = [B][C] / [A]^2 = (0.2)(0.3) / (0.5)^2 = 0.12 / 0.25 = 0.48.

Kp is defined as the partial pressure of products over reactants, raised to the power of their coefficients.

The value of Kp is specific to the reaction conditions and cannot be determined without knowing the initial concentrations or the extent of the reaction.

The gas constant R is 0.0821 L·atm/(K·mol).

The principal quantum number n for the f subshell is 4.

The principal quantum number (n) indicates the energy level of the electron. For 4s, n=4.

In the ground state, the electron is in the first energy level, which corresponds to n=1.

Potassium has the electronic configuration [Ar] 4s1, so the outermost electron is in n=4.

Sodium has an atomic number of 11, and its electron configuration is 1s² 2s² 2p⁶ 3s¹. The outermost electrons are in n=3.

Potassium (K) has an atomic number of 19, and its electron configuration ends in 4s, so the outermost electron has n=4.

The ground state of hydrogen corresponds to n=1.

Sodium has an atomic number of 11, and its outermost electrons are in the n=3 shell.

Potassium has an atomic number of 19, and its outermost electrons are in the n=4 shell.

The universal gas constant R is 0.0821 L·atm/(K·mol).

NaCl dissociates into two ions (Na+ and Cl-), so the van 't Hoff factor (i) is 2.

The van 't Hoff factor (i) is equal to the number of particles the solute dissociates into. For a strong electrolyte that dissociates into 3 ions, i = 3.

The van 't Hoff factor (i) for glucose is 1, as it does not dissociate in solution.

For a non-electrolyte solute, the van 't Hoff factor (i) is 1, as it does not dissociate into ions.

Vapor pressure = P°_solvent * (n_solvent / (n_solvent + n_solute)) = 23.76 * (55.5 / (55.5 + 0.1)) = 22.88 mmHg

Using Raoult's law, P_solution = X_solvent * P°_solvent = (9/10) * 100 mmHg = 90 mmHg.

Vapor pressure lowering = (moles of solute / total moles) * P0 = (1 / (1 + 3)) * P0 = 0.25 P0, so vapor pressure = P0 - 0.25 P0 = 0.75 P0.

Using Raoult's law, the vapor pressure of the solution = (moles of solvent / total moles) * P0 = (10 / 11) * P0 = 0.909 P0.

Using Raoult's law, P_solution = X_solvent * P°_solvent. X_solvent = 3/(1+3) = 0.75, so P_solution = 0.75 * 100 mmHg = 75 mmHg.

Using Raoult's law, the vapor pressure of the solution = (moles of solvent / total moles) * P0 = (3 / (3 + 1)) * P0 = 0.75 P0.

The vapor pressure of a solution containing a non-volatile solute is lower than that of the pure solvent due to the presence of solute particles.

At STP, 1 mole of an ideal gas occupies 22.4 liters.