on adding POCl, according to le chatelier principle, on increasing the concentration of product reaction moves in back ward direction to reestablish equlibrium.so reverse reaction proceeds to establish equlibrium. and when reactoin goes in backward direction, partial pressure of POCl and Chlorine will decreases and partial pressure of POCl3 will increases.
so answer is Only B : The reverse reaction will proceed to establish equlibrium.
32. The reaction system POCls(g) POCI(g)+ Cl2(g) is at equilibrium. Which of the following statements describes...
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)...
At 25°C, the equilibrium constant K for the reaction in the solven 2BrCl = Br2 + Cl2 is 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine? 1.35 x 10-3M 2.70 x 10-3M 8.82 x 10-3 M 9.70 x 10-2 M. none of these choices is correct Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. D. NH4Is) + NH3(g) +HI(g) At 400°C, Kp =...
Q(7) The reaction system POBr3(g) - POBr(g) + Brz(g) is at equilibrium. Which of the following statements describes the behavior of the system if POBr is added to the container? A) The reverse reaction will proceed to establish equilibrium. B) The partial pressures of POBra and POBr will remain steady while the partial pressure of bromine increases. C) The partial pressure of chlorine will increase while the partial pressure of POB decreases. D) The partial pressure of chlorine remains steady...
Consider the following system at equilibrium where AHo--87.9 kJ, and Kc-83.3, at 500 K. PCl3(g) C2(gPCI5(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of KcA. increases B. decreases C. remains the same The value of Qc A. is greater than Kc B. is equal to Kc C. is less than K The reaction must:A. run in the forward direction to reestablish equilibrium B. run in the reverse direction to reestablish equilibrium C....
Consider the following system at equilibrium where H° =
-108 kJ, and Kc = 77.5
, at 600 K:
CO (g) + Cl2(g)
COCl2(g)
If the TEMPERATURE on the equilibrium system is
suddenly increased :
The value of Kc
A. Increases
B. Decreases
C. Remains the same
The value of Qc
A. Is greater than Kc
B. Is equal to Kc
C. Is less than Kc
The reaction must:
A. Run in the forward direction to restablish equilibrium.
B. Run...
Consider the following system at equilibrium where H° =
-87.9 kJ, and Kc =
83.3 , at 500 K:
PCl3(g) +
Cl2(g) PCl5(g)
If the TEMPERATURE on the equilibrium system is
suddenly decreased :
The value of Kc
A. Increases
B. Decreases
C. Remains the same
The value of Qc
A. Is greater than Kc
B. Is equal to Kc
C. Is less than Kc
The reaction must:
A. Run in the forward direction to restablish equilibrium.
B. Run in...
Consider the following system at equilibrium where AH° = -198 kJ, and K. = 34.5, at 1.15*10' K. 2802(g) + O2(g) 2803(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of K A. increases. B. decreases. C. remains the same. The value of Qc A. is greater than K. B. is equal to K C. is less than K The reaction must: A. run in the forward direction to reestablish equilibrium. B. run...
Consider the following system at equilibrium where Delta H° = -108 kJ, and Kc = 77.5, at 600 K. CO(g) + Cl2(g) <---> COCl2(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of Kc A. increases. B. decreases. C. remains the same. The value of Qc A. is greater than Kc. B. is equal to Kc. C. is less than Kc. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run...
For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35 x 10^4. Hydrogen at a partial pressure of 0.700 bar and chlorine at a partial pressure of 0.500 bar are placed in a vessel at 800oC and allowed to equilibrate. Find the final partial pressures of all three gases in this reaction in bar
For the reaction H2(g) +
Cl2(g) 2 HCl(g), the
equilibrium constant K at 800oC is 4.35 x
104.
Hydrogen and chlorine, each at a partial pressure of 0.700 bar,
are placed in a vessel at 800oC and allowed to
equilibrate. Find the final partial pressures of all three gases in
this reaction.
p(H2) = bar
p(Cl2) =
. bar
p(HCl) =
bar