The problem explains behaviour of phosphorus pentachloride (PCl5) at various temperatures from the point of bonding and structure.

PCl5 is a white solid, which volatilises at 160oC and melts at 148oC under pressure. Molten PCl5 conducts an electric current readily. At 180oC PCl5 vapour has a density of 9.3 g/L corrected to the standard conditions. At 250oC a sample of PCl5 exerts a pressure, which is twice the expected value. Discuss these observations and ...continues

Setting up pressure equations.

Set up the equations to solve: P air (torr) : P H2O (torr) : change of H vap: and lnP.

Working with rates of formation given reaction rates.

If NOCl is reacting at a rate of 0.24 mol/L.s, what is the rate of formation of Cl2(g)? 2NOCl(g) --> 2NO(g) + Cl2

Calculating the half life of a reaction.

For the first order reaction below, the intial concentration of A is 0.280M. If the concentration of A decreases to 0.0700 after 22.8 hours, what is the half-life of the reaction? A-->B rate=k[A]

Calculating the activation energy given the rate constant and change in temperature.

For a certain reaction, the rate constant doubles when the temperature is increased from 25 degrees Celsius to 41 degrees Celsius. What is the activation energy for this reaction? (R=8.31J/mol.K)

Working with half lives to determine the time required to reach a certain percentage of its initial concentration.

A first order reaction has a half-life of 157 seconds. How much time is required for the reactant to be reduced to 12.5% of its initial concentration?

Identifying a catalyst in a reaction.

The elementary steps for the catalyzed decomposition for dinitrogen monoxide are shown below. Identify the catalyst. NO(g)+N2O(g)--->N2(g)+NO2(g) 2NO2(g)-->2NO(g)+O2(g)

Calculating the change in the rate constant when temperature is decreased.

For a certain reaction, the activation energy is 52.1kJ/mole. By what ratio will the rate constant change if the temperature is decreased from 175 degrees Celsius to 75 degrees Celsius?

Calculating the time required for a reaction to be reduced by a certain percentage given the half life.

A first order reaction has a half-life of 2.10 hours. How much time is required for the reactant to be reduced to 33.0% of its initial concentration?

Calculating the partial pressure of a gas at equilibrium given the equilibrium constant.

At a given temperature, the equilibrium constant (Kp) for the decomposition of dinitrogen dioxide is 0.172. If 0.224atm N2O4 is sealed in a flask, what partial pressure of NO2 will exist at equilibrium?