Le Chatelier's principle states that if a system at equilibrium is subjected to a change, the system will adjust to counteract that change.

The Beer-Lambert Law is expressed as A = εcl, where A is absorbance, ε is molar absorptivity, c is concentration, and l is path length.

The Beer-Lambert Law relates the absorbance of light to the concentration of a solution, allowing for concentration determination.

The bond angle in water is approximately 104.5 degrees due to the repulsion of the two lone pairs.

The bond angle in H2O is approximately 104.5 degrees due to the bent shape of the molecule caused by the two lone pairs on the oxygen atom.

Bond order = (number of bonding electrons - number of antibonding electrons) / 2. For 10 electrons, if all are bonding, bond order = 10/2 = 5. If 2 are antibonding, bond order = (10-2)/2 = 4. The most stable configuration gives a bond order of 2.

Bond order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (5 - 5) / 2 = 0.

Bond order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (10 - 4) / 2 = 3.

Bond order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (3 - 1) / 2 = 1.

Bond order = (12 - 4) / 2 = 4. The bond order for O2 is actually 2, but this question is hypothetical.

N2 has 10 bonding electrons and 2 antibonding electrons, so bond order = (10 - 2) / 2 = 4 / 2 = 2.

O2 has 12 total valence electrons. The bond order is calculated as (number of bonding electrons - number of antibonding electrons) / 2 = (10 - 2) / 2 = 4 / 2 = 2.

O2 has 12 total electrons, with 10 in bonding orbitals and 2 in antibonding orbitals. Bond order = (number of bonding electrons - number of antibonding electrons) / 2 = (10 - 2) / 2 = 4 / 2 = 2.

In an endothermic reaction, heat is absorbed from the surroundings, resulting in a positive change in enthalpy (ΔH > 0).

In an exothermic reaction, heat is released, resulting in a negative change in enthalpy (ΔH < 0).

ΔH = Σ(bond enthalpies of reactants) - Σ(bond enthalpies of products) = [2(436) + 498] - [4(463)] = −572 kJ.

The change in enthalpy for the reaction is equal to the standard enthalpy of formation of H2O(l), which is -285.8 kJ/mol.

The change in enthalpy for the reaction is equal to the standard enthalpy of formation of H2O(l), which is -285.83 kJ/mol.

At constant pressure, the change in enthalpy (ΔH) is defined as the heat absorbed or released by the system.

2-methylpropan-1-ol is commonly known as isobutanol.

Alkenes are commonly used in the production of plastics, such as polyethylene.

pOH = 14 - pH = 14 - 11 = 3. [OH-] = 10^-pOH = 10^-3 M.

The conjugate base of H2SO4 is HSO4-, formed when H2SO4 donates a proton (H+).

In a tetrahedral complex, the coordination number is 4, as there are four ligands surrounding the central metal atom.

In an octahedral complex, the coordination number is 6, as there are six ligands surrounding the central metal atom.

The coordination number is defined as the number of ligand atoms that are bonded to the central metal atom. In this case, with six ligands, the coordination number is 6.

In the complex ion [H2O]2+, the coordination number of hydrogen is 2.

In the complex [Ni(H2)6], the coordination number of hydrogen is 6, as there are six hydrogen ligands coordinated to nickel.

The coordination number is determined by the number of ligands attached to the central metal ion. In this case, there are six NH3 ligands, giving a coordination number of 6.

The coordination number of copper in [Cu(NH3)4]SO4 is 4, as it is surrounded by four ammonia ligands.