Removing Cl2 decreases its concentration, causing the equilibrium to shift to the right to produce more Cl2.

'a' accounts for the attractive forces between particles, while 'b' accounts for the volume occupied by the gas particles in the van der Waals equation.

The indicator in titration provides a visual signal of the endpoint, indicating when the reaction is complete.

According to the Beer-Lambert Law, higher absorbance indicates a higher concentration of the absorbing species in the solution.

According to Beer-Lambert Law, higher absorbance indicates a higher concentration of the absorbing species.

A higher absorbance indicates a higher concentration of the analyte, as per the Beer-Lambert Law.

A higher absorbance value indicates a higher concentration of the analyte, according to Beer-Lambert law.

A higher molar absorptivity indicates that a substance is more efficient at absorbing light at a given wavelength.

A peak at 260 nm in UV-Vis spectroscopy typically indicates the presence of nucleic acids, as they absorb light at this wavelength.

A peak at 280 nm typically indicates the presence of proteins, particularly due to the absorbance of aromatic amino acids.

A peak in the absorbance spectrum indicates the presence of a specific ion or compound that absorbs light at that wavelength.

A peak in the absorption spectrum corresponds to a specific electronic transition of electrons within the molecule.

A shift in the absorption peak in UV-Vis spectroscopy often indicates a change in molecular structure, such as the formation of new bonds or changes in electronic transitions.

The Beer-Lambert law relates absorbance to concentration, indicating that absorbance increases linearly with concentration of the absorbing species.

Increasing the path length of the sample cell increases the absorbance according to the Beer-Lambert Law, as absorbance is directly proportional to path length.

Primary valence refers to the oxidation state of the central metal atom in a coordination compound.

Ligands act as electron donors to the metal ion, forming coordinate covalent bonds and stabilizing the coordination complex.

Hydrogen acts as a reducing agent in the extraction of metals from their ores, such as in the reduction of metal oxides.

BF3 has a trigonal planar geometry with bond angles of approximately 120°.

In HCl, hydrogen can act as a Lewis acid by accepting an electron pair.

In NaH (sodium hydride), hydrogen has an oxidation state of -1.

In SF6 (sulfur hexafluoride), the sulfur atom is sp3d2 hybridized, allowing it to form six sigma bonds with fluorine atoms.

CH4 has a tetrahedral geometry with bond angles of approximately 109.5 degrees.

In CH4, the carbon atom has four bonding pairs and no lone pairs, leading to sp3 hybridization.

In the complex [Fe(H2O)6]2+, water (H2O) acts as a ligand, coordinating with the iron ion.

Hydrogen bonding occurs in H2O due to the presence of highly electronegative oxygen atoms bonded to hydrogen, creating strong dipole interactions.

C2 has a triple bond between the two carbon atoms, resulting in the shortest bond length compared to the others.

C2H4 has a double bond between the carbon atoms, indicating sp2 hybridization.

SiCl4 has four bonding pairs and no lone pairs, leading to sp3 hybridization of the silicon atom.

Hydrogen reduction is a process where hydrogen gas is used to reduce metal ores to their metallic form.