Physical Chemistry Answers

The following Table 1 shows kinetic study values obtained from second order the gas phase reaction.

X₂  + H₂    → 2HX

Table 1

T (K) k(cm³ mol^-1 s^-1

600 4.6 x 10²

700 9.7 x 10³

800 1.3 x 10⁵

1000 3.1 x 10⁶

[Average molar mass of reactant is 128 g mol^-1]

Find:

i. The collision frequency at 700 K (in m³ s^-1).

ii. The collisions diameter.

The following mechanism is for gas phase pyrolysis of methane:       

 CH4= ∙CH3 + ∙H

∙CH₃ + CH₄        =      C₂H₆ + ∙H

∙H + CH₄        =      ∙CH₃ + H₂

   H + ∙CH₃ + M         =     CH₄ + M

 Derive the rate law for the formation of C₂H₆ 

The e.m.f. of the following cell reaction is  0.6753 V at 25 ℃ and 0.6915 V at

0 ℃.

Cd(s) | CdCl₂.5H₂O(saturated) || AgCl(s) | Ag(s)

(i) Give the balance for the cell reaction

(ii) Calculate the free energy G, enthalpy H and entropy S, change of the cell reaction at 25 ℃.   

Show graphically reversible work of compression is minimum work.

the rate constant for alkali hydrolysis of bromopenta amine cobalt II [C₂(NH₃)₅Br]²⁺ depends on ionic strength as tabulated below. what can be said about the activated complex in the rate determining stage?

I 0.005 0.010 0.015 0.020 0.025 0.030

k/k_o 0.718 0.631 0.562 0.515 0.475 0.447

Show and explain why that the final volume in adiabatic expansion of an

ideal gas is smaller than the isothermal expansion for the same change in

pressure.

If a gas occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm

A metal tank contains three gases:  oxygen, helium, and nitrogen.  If the partial pressures of the three gases in the tank are 35 atm of O2, 5 atm of N2, and 25 atm of He, what is the total pressure inside of the tank?

A weather balloon is released from the ground where it had a volume of 75.0 L. The balloon is captured at the top of the CN tower and now is found to have a volume of 96.5 L where the air pressure is measured to be 93 kPa. What was the pressure inside the balloon on the ground?

 gas occupies 900.0 mL at a temperature of 27.0 °C. What is the temperature if the same gas now has a volume of 1.75 L?