flask at 150°C to reach equailbrium in the following at is the newe has increase
ID: 711400 • Letter: F
Question
flask at 150°C to reach equailbrium in the following at is the newe has increased by 1.464 × 104 atin. If the P,o is then increased to "being ad otal pressure has incressed by 1.464 x 10+ atm froma starting point of Cl is placed in a At equilibrium, the total pressure mial pressure 1.89 × 102 atm, the new a. What does 1 10aium, the it mean that the total pressure partial pressure of NH? H.Ce that s task? (Remember total pressure is the sum of partial pressures) b. What is the equilibrium partial pressures of the gases? C Wh at is the value of K, based upon this information? (Write the e value of K, based upon this information? (Write the equilibrium constant d. A stress is a pplied to the system (increasing Pato 1.89×10-atm, write an ce table representing e addition of a new initial amount of HCl. (The stress on the systeml) Solve the ice table for the partial pressure of NH3.Explanation / Answer
Initially enough NH4Cl means NH4Cl is in solid form it will contribute to the pressure in the container the gas formed by the reaction will contribute to the pressure enough NH4Cl means it can form gases in mentioned molar ratio such that they will give a total pressure of 1.464 * 10-2 atm
NH4Cl (s) <---> NH3 (g) + HCl (g)
1 mole 1 mole 1 mole
as equal amount of NH3 and HCl will be formed when the reaction starts with no NH3 and HCl and just from enough NH4Cl then the total pressure in the vessel will have equal contribution from both gases
total pressure = 1.464 * 10-2 atm = P
partial pressure NH3 = 1.464 * 10-2 atm * 0.5 = 0.732 * 10-2 atm
partial pressure HCl = 0.732 * 10-2 atm
Kp = pNH3 * pHCl = 0.732 * 10-2 atm * 0.732 * 10-2 atm = 0.536 * 10-2 Answer (c)
NH4Cl NH3 HCl
Intial - 1.89 0.732
convert x -x -x
equilibrium x 1.89-x 0.732-x
Kp = 0.536 * 10-2 = (1.89 * 10-2 -x) (0.732 * 10-2 -x)
x = 0.603 * 10-2 atm
pNH3 = 0.732 * 10-2 - 0.603 * 10-2 = 0.129 * 10-2 atm
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