POCl3(l) <--> POCl3 (g)
(a) Calculate ΔGº for the reaction at 25ºC.
(b) Calculate the Kp of the vaporization of POCl3(l) to POCl3(g) at 25ºC.
(c) Determine the partial pressure of POCl3 at 25ºC?
POCl3(l) <--> POCl3 (g) (a) Calculate ΔGº for the reaction at 25ºC. (b) Calculate the Kp...
. Consider the reaction: POCl3 (l) --> POCl3 (g) (a) Calculate ΔGº for the reaction at 25ºC. (b) Calculate the Kp of the vaporization of POCl3(l) to POCl3(g) at 25ºC. (c) Determine the partial pressure of POCl3 at 25ºC?
The reaction system POCL3(g) -><- POCL(g) + Cl2(g) is at equilibrium. Which of the following statements describes the behavior of the system if POCL is added to the container? A) The reverse reaction will proceed to establish equilibrium. B) The partial pressure of cholrine will increase while the partial pressure of POCL decreases. C) The partial pressure of chlorine remains steady while the partal pressures of POCL3 and POCL increase D The forward reaction will proceed to establish equilibrium. E)...
For the reaction 2 A (g) – B (g), Kp = 0.00565 at 298 K. When AG = 8.35 kJ/mol, what is the partial pressure of B when the partial pressure of A is 2.00 atm for this reaction at 298 K.
Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give the following information (298.15 K) NO (g) +1/2Br2(g) NOBr(g) Ke 4.5 2 NO (g)N2(g) 02(g) Ke 3.0 x 102 5. For the BrCl decomposition reaction 2BrCl(g) Br2(g Cl2(g) Initially, the vessel is charged at 500 K with BrCl at a partial pressure of 0.500 atm. At equilibrium, the partial pressure of BrC is 0.040 atm. Calculate Kp value at 500K
Consider the...
At 400K, the equilibrium constant for the reaction Br2(g) + Cl2(g) ⇌ 2BrCl(g) is KP = 7.0. A closed vessel at 400K is charged with 1.00 atm of Br2(g), 1.00 atm of Cl2(g), and 2.00 atm of BrCl(g). Use Q to determine which of the statements below is true. A. The equilibrium partial pressure of BrCl(g) will be less than 2.00 atm B. The reaction will go to completion since there are equal amounts of Br2 and Cl2 C. At...
QUESTION 4 At a certain temperature, Kp for the reaction 12(g)-=> 2 l(g) is 0.000778 Calculate the value of Kp for the reaction 21(g)s=> 12(g)
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1346 torr and a H2O partial pressure of 1762 torr at 2000 K. A.) Calculate the equilibrium partial pressure of CO2. B.) Calculate the equilibrium partial pressure of H2.
1. calculate Kp for the reaction C(s) + Co2(g) = 2Co(g at 1300 k and 1 atm, the equilibrium mixture contains 85% co and 10.5% co2 by volume. 2. calculate the partial pressure of Co2 if Pco is changed to 10^-3 ATM.
1. The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <----> PCl3(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.00 atm at 500 K. PPCl5 = atm PPCl3 = atm PCl2 = atm 2. The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K: NH4I(s) <----> NH3(g) + HI(g) Calculate the equilibrium partial pressure of HI when...
Consider the reaction: CO(g) + H2O(g) -><- CO2(g) +
H2(g)
Kp = 0.0871 at 1000 K
A reaction mixture originally contains a CO partial pressure
of 1744 torr and a H2O partial pressure of 766 torr at 1000 K.
Caluculate the equilibrium partial pressures of each of the
products
6) (10 points) Consider the reaction: CO(g) + H2O(g) = CO2(g) + H2(g) Kp = 0.0871 at 1000 K A reaction mixture initially contains a CO partial pressure of 1 744...