Question

In: Chemistry

In chemical equation H2 (g) + I2 (g) ⇌ 2HI (g) the equilibrium constant Kp depends on (a) total pressure (b) catalyst used (c) amount of H2 and I2 (d) temperature

In chemical equation H2 (g) + I2 (g) ⇌ 2HI (g) the equilibrium constant Kp depends on___________.

(a) total pressure

(b) catalyst used

(c) amount of H2 and I2

(d) temperature

Solutions

Expert Solution

Answer : (d) temperature

Explanation :

For the reaction,

H2(g) +I2(g) ⇌2HI(g)

The number of moles of gaseous reactants on reactant sude is 2 that is equal to the number of moles of gaseous products.

The equilibrium constant Kp is independent of 

  1. Total pressure
  2. Catalyst
  3. Amount of I2 and H2
  4. Catalyst 
  5. Volume 
  6. Pressure 
  7. Concentration of reactant and product. 

 


d) temperature 

Related Solutions

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature,...
At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature, 0.7 mol of H2 and 0.7 mol of I2 were placed in a 1 L container. What is the concentration of HI present at equilibrium?
For the reaction H2(g) + I2(g) ↔ 2HI the value of the equilibrium constant is 25....
For the reaction H2(g) + I2(g) ↔ 2HI the value of the equilibrium constant is 25. Starting with 1.00mol of each reactant in a 10.L vessel, how many moles of HI will be present at equilibrium?
At 500K, the equilibrium constant, Keq, is 155 for the reaction H2(g) + I2(g) ↔ 2HI(g)....
At 500K, the equilibrium constant, Keq, is 155 for the reaction H2(g) + I2(g) ↔ 2HI(g). Calculate the equilibrium constant for the reaction  2H2(g) + 2I2(g) ↔ 4HI(g), 1/2H2(g) + 1/2I2(g) ↔ HI(g), and 2HI(g)  ↔ H2(g) + I2(g).
Consider the following reaction: H2(g)+I2(g)?2HI(g) The data in the table show the equilibrium constant for this...
Consider the following reaction: H2(g)+I2(g)?2HI(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature Kp 150 K 1.4×10?6 175 K 4.6×10?6 200 K 3.6×10?2 225 K 1.1 250 K 15.5 Use the data to find ?H?rxn and ?S?rxn for the reaction.
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2...
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2 (g) ---> 2 HI (g) Kc= 53.3 At this temperature, 0.600 mol of H2 and 0.600 mol of I 2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?
At 500 °C, hydrogen iodide decomposes according to 2HI(g)↽−−⇀H2(g)+I2(g)2HI(g)↽−−⇀H2(g)+I2(g) For HI(g)HI(g) heated to 500 °C in...
At 500 °C, hydrogen iodide decomposes according to 2HI(g)↽−−⇀H2(g)+I2(g)2HI(g)↽−−⇀H2(g)+I2(g) For HI(g)HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2]=0.400 M[H2]=0.400 M , [I2]=0.400 M[I2]=0.400 M , and [HI]=3.38 M[HI]=3.38 M . If an additional 1.00 mol of HI(g)HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached? [HI]= [H2]= [I2]= Please help and show work!
The equilibrium constant for the chemical equation is Kp = 24.6 at 181 �C. Calculate the...
The equilibrium constant for the chemical equation is Kp = 24.6 at 181 �C. Calculate the value of the Kc for the reaction at 181 �C. N2 (g) + 3H2 (g) ---> 2NH3 (g) K_c = ?
Find the temperature in ºC at which Kp = 43.7 for the reaction H2(g) + I2(g)...
Find the temperature in ºC at which Kp = 43.7 for the reaction H2(g) + I2(g) ⇌ 2 HI(g). Use ∆Hºrxn and ∆Sºrxn to calculate and assume that they are independent of temperature. Use the thermodynamic data in the appendix of your textbook; I have provided the needed appendix on BlackBoard for your convenience. Report your answer to zero places past the decimal.
The equilibrium constant Kc is 54.3 at 430°C for the following reaction: H2(g) + I2(g) ⇌...
The equilibrium constant Kc is 54.3 at 430°C for the following reaction: H2(g) + I2(g) ⇌ 2HI(g) Initially, 0.90 M H2, I2, and HI are introduced into a 5.0-L flask and allowed to come to equilibrium. What are the equilibrium concentrations of H2, I2, and HI in the flask? (10 points) (Does the size of flask matter since Molarity is given?)
Consider the following reaction: H2(g) + I2(g) ⇌ 2HI(g) At a particular temperature, a reaction mixture...
Consider the following reaction: H2(g) + I2(g) ⇌ 2HI(g) At a particular temperature, a reaction mixture at equilibrium contains pressures of H2 = 0.958 atm, I2 = 0.877 atm, and HI = 0.020 atm. At the same temperature, a second reaction mixture (not at equilibrium) contains pressures of H2 = 0.621 atm, I2 = 0.621 atm, and HI = 0.101 atm. What will be the partial pressure of HI when the second reaction mixture reaches equilibrium? a) 0.0144 atm b)...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT