Boyle's Law states that the pressure of a gas is inversely proportional to its volume at constant temperature (P1V1 = P2V2).

Boyle's Law states that the pressure of a gas is inversely proportional to its volume at constant temperature (P1V1 = P2V2).

For a first-order reaction, the rate is directly proportional to the concentration of the reactant.

According to the Arrhenius equation, the rate constant increases with temperature due to the exponential dependence on the negative activation energy divided by temperature.

The Arrhenius equation states that the rate constant k is related to temperature T and activation energy Ea by k = Ae^(-Ea/RT), where A is the pre-exponential factor.

According to the Arrhenius equation, k increases with increasing temperature due to the exponential dependence on the negative activation energy divided by temperature.

In a first-order reaction, the rate is directly proportional to the concentration of the reactant.

A catalyst lowers the activation energy, allowing the reaction to proceed faster without being consumed.

The cathode is the electrode where reduction occurs, gaining electrons from the external circuit.

The salt bridge maintains charge balance by allowing ions to flow between the two half-cells, preventing charge buildup.

With 5 bonding pairs and 1 lone pair, the molecular shape is square pyramidal.

The NH4+ ion has a tetrahedral shape due to four bonding pairs around the nitrogen atom.

PCl5 has five bonding pairs and no lone pairs, resulting in a trigonal bipyramidal shape.

The critical point marks the end of the liquid-gas phase boundary, beyond which distinct liquid and gas phases do not exist.

The equilibrium constant (K) expresses the ratio of the concentrations of products to reactants at equilibrium, indicating the extent of the reaction.

The Faraday constant represents the charge of one mole of electrons, approximately 96485 C/mol.

Gibbs free energy indicates the spontaneity of a process; a negative change in G suggests a spontaneous reaction.

ΔG indicates whether a reaction is spontaneous (ΔG < 0) or non-spontaneous (ΔG > 0).

Gibbs free energy (G) indicates the spontaneity of a process; a negative change in G (ΔG < 0) suggests a spontaneous reaction.

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 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 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.