equil_practice-1 - 4. At 1000 K, the equilibrium mixture...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Practice Problems on Equilibrium All of the problems given here assume the use of proper thermodynamic equilibrium constants (phrased in terms of activities). 1. Write equilibrium constant expressions for the following reactions both in terms of activities and in terms of the observables (pressure, concentration, mole fraction) which underlie them. (a) C s CO 2 g 2CO g (b) CO 2 g H 2 O l H 2 CO 3 aq (c) NH 4 2 CO 3 s 2NH 3 g CO 2 g H 2 O g (d) Ba OH 2 s Ba 2 aq 2OH aq 2. For the reaction I 2 g 2I g , K 2 3 10 10 at 500 K. Analysis of a mixture kept at 500 K shows that the partial pressure of I 2 is 0.87 atm while the partial pressure of iodine atoms is 8 2 10 7 atm. Is the mixture in equilibrium? If not, in what direction is the reaction spontaneous? 3. When the reaction PCl 5 g PCl 3 g Cl 2 g reaches equilibrium at 250 C, the partial pres- sures of the reactant and products are as follows: P PCl 5 1 8 10 3 atm, P PCl 3 0 56atm, P Cl 2 0 17atm. What is the equilibrium constant for the reaction at this temperature?
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: 4. At 1000 K, the equilibrium mixture for the gas-phase reaction of sulfur dioxide with oxygen forming sulfur trioxide contains 3 77 10 3 mol L of sulfur dioxide, 4 13 10 3 mol L of sulfur trioxide and 4 30 10 3 mol L of oxygen. Calculate the equilibrium constant. 5. The equilibrium constant for the dissociation of iodine molecules into iodine atoms (I 2 g 2I g ) is 0.31 at 1000 K. If 25 g of iodine is placed in a 12 L flask at 1000 K, what are the equilibrium pressures of iodine molecules and atoms? 6. The equilibrium constant for the reaction COBr 2 g CO g Br 2 g at 73 C is 5.4. If 0.015 mol of COBr 2 is warmed to 73 C in a 2.5 L flask, what is the final pressure reached? Hint: The pressure at any time is the sum of the partial pressures of all gases present....
View Full Document

Ask a homework question - tutors are online