The first time I asked I was given the answer 0.686 atm, but it says it is incorrect.
Thanks!
The first time I asked I was given the answer 0.686 atm, but it says it...
Consider the following reaction. 2A(g) 근 B(g) Kp = 2.43 × 10-5 at 500 K If a sample of A(g) at 3.90 atm is heated to 500 K, what is the pressure of B(g) at equilibrium? Number atm
Consider the following reaction.If a sample of A(g) at 3.50 bar is heated to 500 K, what is the pressure of B(g) at equilibrium? 2A(g) <--> B (g) Kp = 2.27 x 10^-5 at 500K Pb = ____ bar
Consider the following reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and B for each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions. Given: Kp= 1.6×105 , find Pa, Pb; Given Kp= 2.0×10−4, find Pa, Pb. I can't tell how to get the appropriate x values and equations for equilibrium...
Having problem in solving 3 (iii) Consider the following reaction at equilibrium at 298 K 2Ag(s) 2HC(g)2AgCl(s) Hag Given the following data at 298 K 4 92.21 95 18 126 90 AHkmole) (i) Calculate Δ. ΔΗ , AS and Kp for the reaction at 298 K () Calculate Kp at 500 K w)If no moles of HCI are present initially, caloulate the partial pressure of H2 at equilibrium at 298 K taking α to be the fraction of dissociation and...
Consider the reaction. 2 A(g) + B(g) K, = 2.02 x 10-6 at 500 K If a sample of A(R) at 3.80 atm is heated to 500 K, what is the pressure of B(g) at equilibrium? atm
Consider the reaction. 2 A(g) – B(g) K = 5.90 x 10-5 at 500 K If a sample of A(g) at 1.50 atm is heated to 500 K, what is the pressure of B(8) at equilibrium? P₂ = atm
Consider the reaction. 2A(g)↽−−⇀B(g)?p=1.17×10−5at 500 K If a sample of A(g) A ( g ) at 3.30 atm 3.30 atm is heated to 500 K, 500 K , what is the pressure of B(g) at equilibrium? atm
Consider the reaction. 2 A ( g ) − ⇀ ↽ − B ( g ) K p = 9.80 × 10 − 5 at 500 K If a sample of A ( g ) at 4.90 atm is heated to 500 K , what is the pressure of B ( g ) at equilibrium?
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...
H2 at 1.75 atm and O2 at 0.75 atm are placed in a container at 200 degree C. A spark causes the reaction to form H2O (g). At equilibrium the total pressure is 1.90 atm. PLEASE SHOW WORK. a. Calculate Kp (answer: 32) b. Calculate Kc (answer: 1.2 x10^3)