Boiling point elevation = i * K_b * m = 2 * 0.512 * 0.5 = 0.512 °C; Boiling point = 100 + 0.512 = 100.512 °C

In methane, the bond angle is approximately 109.5 degrees due to its tetrahedral geometry.

In a tetrahedral geometry, the bond angles are approximately 109.5 degrees.

In a trigonal planar geometry, the bond angles are 120 degrees.

The bond angle in H2O is approximately 104.5 degrees due to the two lone pairs on oxygen.

The bond angle in H2O is approximately 104.5 degrees due to the two lone pairs on oxygen.

CO has a bond order of 3, calculated as (10 bonding - 3 antibonding)/2.

O2- has a bond order of 1, calculated as (10 bonding electrons - 7 antibonding electrons)/2 = 1.

B2 has a bond order of 1, calculated as (2 bonding - 0 antibonding)/2.

B2 has a bond order of 1, calculated from its molecular orbital configuration.

CO has a bond order of 3, calculated as (10 bonding electrons - 2 antibonding electrons)/2 = 3.

He2 has a bond order of 0, as it has no net bonding electrons.

N2 has a bond order of 3, calculated as (10 bonding - 0 antibonding)/2 = 3.

O2 has 12 total electrons, leading to a bond order of (10 bonding - 6 antibonding)/2 = 1.

In an endothermic reaction, heat is absorbed from the surroundings, resulting in a positive change in enthalpy.

In an exothermic reaction, heat is released, resulting in a negative change in enthalpy.

In an isothermal process, the temperature remains constant, and for an ideal gas, the change in enthalpy is zero.

The change in entropy for an isothermal and reversible expansion of an ideal gas is given by ΔS = nR ln(V2/V1). For 1 mole, n = 1, hence ΔS = R ln(V2/V1).

The change in entropy for an isothermal expansion of an ideal gas is given by ΔS = nR ln(V2/V1). For 1 mole, it simplifies to ΔS = R ln(V2/V1).

The oxidation state of carbon changes from -4 in CH4 to +4 in CO2.

Mass of KCl = 0.5 moles × 74.5 g/mol = 37.25 g. Concentration = 37.25 g / 1.5 L = 24.83 g/L.

Molality (m) = moles of solute / kg of solvent = 5 moles / 3 kg = 1.67 m.

Molarity (M) = moles of solute / liters of solution = 0.5 moles / 1.5 L = 0.33 M.

PPM = (mass of solute in grams / volume of solution in liters) * 10^6 = (1 g / 1 L) * 10^6 = 1000 ppm.

Molarity (M) = moles of solute / liters of solution = (10 g / 58.5 g/mol) / 0.5 L = 0.34 M.

[H+] = 10^(-pH) = 10^(-3) = 0.001 M

The critical point is where the liquid and gas phases become indistinguishable.

The critical temperature is the temperature above which a gas cannot be liquefied, regardless of the pressure applied.

The critical temperature is the temperature above which a gas cannot be liquefied.

A catalyst does not affect the equilibrium constant; it only speeds up the rate at which equilibrium is reached.