Physical Chemistry Answers

Calculate the equilibrium constant 1.000mol of H(g) and 1.000mol of Iodine vapour are introduced into a 5.00liter sealed glass, the mixture is heated to a certain temperature, at equilibrium the mixture is found to contain 1.500mol of HI

1. What are the Concentration of H(g) and I(g) at equilibrium

2. Calculate the equation constant kc

Equilibrium Exercise #1 A flask is charged with 2.00 atm of nitrogen dioxide and 1.00 atm of dinitrogen tetroxide at 25 oC and allowed to reach equilibrium. When equilibrium is established, the partial pressure of NO2 has decreased by 1.24 atm. (a) What are the partial pressures of NO2 and N2O4 at equilibrium? (b) Calculate Kp and Kc for following reaction at 25 oC.

2 NO2(g) ⇄ N2O4(g)

(Answer: Kp = 2.80; Kc = 68.6)

10g of the gas as 17^oC are compressed adiabatically and reversibly from 8 to 5 liters. calculate the final temperature and the work done on the gas. what are ΔU and ΔH for the process (Cp=3/2R and R= 8.314)

one mole of gas allowed to expand reversibly i.e. against confining pressure that is at all times infinitesimally less than the gas pressure, from an initial pressure of 10atm to a final pressure of 0.4atm, the temperature being kept constant at 0^oC.

a. how much work is done by the gas?

b. what is the change in initial energy and enthalpy?

c. How much heat is absorbed?

1 mole of an ideal gas is allowed to expand against a piston that supports 0.4atm. the initial pressure was 10atm and final pressure is 0.4atms, the temperature being constant at 0^oC.

a. How much work is done by the gas during the expansion?

b. what is the change in internal energy and in the enthalpy of the gas

c. How much heat is absorbed?

Calculate the number of moles and molarity of n/2 500 ml solution of H2SO4

A flask is charged with 2.00 atm of nitrogen dioxide and 1.00 atm of dinitrogen tetroxide at 25 oC and allowed to reach equilibrium. When equilibrium is established, the partial pressure of NO2 has decreased by 1.24 atm. (a) What are the partial pressures of NO2 and N204 at equilibrium? (b) Calculate Kp and Kc for following reaction at 25 2 NO2(g) N204(g)

6.300 mole of Hd Is Introduced lute & 1. volitere seslect fast andl Theated to a certain temperature. Under this condition HI decompses to precluce H. and In until an equilibrium ls established. An 9 Lyses of the equilibrium moxture shows that 0.105 mole of HI lus

decompuseet - Calculate the quilibrium. Constand Concentration of the Is and HI and the equilibris Constant ke for the following reaction

  A flask is charged with 2.00 atm of nitrogen dioxide and 1.00 atm of dinitrogen tetroxide at 25 oC and allowed to reach equilibrium. When equilibrium is established, the partial pressure of NO2 has decreased by 1.24 atm. (a) What are the partial pressures of NO2 and N2O4 at equilibrium? 

  (b) Calculate Kp and Kc for following reaction at 25 oC. 

      2 NO2(g) ⇄ N2O4(g)

Calculate the calorific value of coal sample from the following data:

Mass of coal: 1g, water and water equivalent of calorimeter: 2 Kg

Specific heat of water: 4.187 KJKg-1C

-1

and rise in temperature: 4.8oC