UV-Vis spectroscopy is significant in qualitative analysis as it can identify the presence of colored ions based on their absorbance characteristics.

E° = E°(Cu²⁺/Cu) - E°(Zn²⁺/Zn) = 0.34 V - (-0.76 V) = 1.10 V.

E°cell = E°cathode - E°anode = 0.34 V - (-0.76 V) = 1.10 V.

The standard electrode potential for the reduction of Ag⁺ to Ag is 0.80 V.

The standard electrode potential indicates the tendency of a species to gain electrons and be reduced.

The standard electrode potential is the voltage measured under standard conditions (1 M concentration, 1 atm pressure, and 25°C).

The standard electrode potential for the reduction of copper ions to copper is +0.76 V.

The standard enthalpy change for the formation of CO2(g) is directly given as ΔH° = -393.5 kJ.

At equilibrium, the forward and reverse reactions occur at the same rate, resulting in no net change in enthalpy (ΔH = 0).

The standard enthalpy change for the combustion of CH4 is calculated as ΔH = [2(-393.5) + (-285.8)] - [1(0)] = -890.3 kJ/mol.

The standard enthalpy change for the formation of water (H2 + 0.5 O2 -> H2O) is -285.8 kJ/mol.

The standard enthalpy change is 2 * (-241.8 kJ) = -483.6 kJ for the formation of 2 moles of H2O(g).

Standard enthalpy change (ΔH°) is measured at standard conditions, which are defined as 1 atm pressure and 25°C (298 K).

The standard enthalpy change of formation for elements in their standard state is defined as 0 kJ/mol.

The standard enthalpy of formation for any element in its standard state is defined as zero.

The standard reduction potential for the half-reaction H2 → 2H+ + 2e- is defined as 0.00 V.

Standard temperature and pressure (STP) for gases is defined as 0°C (273.15 K) and 1 atm (101.3 kPa).

The configuration (2R,3S) indicates that the second carbon is R and the third carbon is S.

(R)-2-butanol has the R configuration at the chiral center.

The chiral center in 2-bromo-3-methylpentane has the highest priority groups arranged in a clockwise manner, giving it an R configuration.

2-bromobutane can exist as two enantiomers, R and S, due to the presence of a chiral center at the second carbon.

2-Butanol has a chiral center and can exist as both R and S enantiomers.

When the two methyl groups are on opposite sides of the double bond, the configuration is called trans.

When the two methyl groups are on the same side of the double bond, the configuration is referred to as cis.

The S_N2 reaction will invert the configuration, resulting in the (S) configuration for the product.

The SN2 reaction will invert the configuration of (R)-2-bromobutane, resulting in the (S) configuration.

SN2 reactions result in inversion of configuration at the carbon center where the nucleophile attacks, leading to a stereochemical change.

The addition of H2 across an alkene occurs via syn addition, resulting in both hydrogens adding to the same side of the double bond.

Only one product is formed when 1,2-dimethylbenzene is substituted at the 4-position, as the two methyl groups are in positions that do not create stereoisomers.

Electrophilic substitution at the 5-position of o-xylene leads to two diastereomers due to the presence of two chiral centers.