2) For the following reaction:NH4HS(s)<->NH3(g) + H2S (g) Kc=8.5x10^-3
At any given point the reaction mixture has solid NH4HS, NH3 at 0.166M and H2S at 0.166M.
3) Consider the following reaction: CH3OH (g) <-> CO (g) + 2H2 (g) deltaH=+90.7 kJ/mol
Select what disturbances you can do to shift the reaction to the right (check all that apply)
The reaction CO2(g) + C(s) <-> 2CO(g) has a Kp=5.78 at 1200k Delta n for the...
1) For the following reaction: SO2Cl2(g)<-> SO2(g) + Cl2 (g) Kp=2.91x10^3 at 298K In the reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of CL2 is 285 torr. The partial pressure of SO2Cl2 is [x]torr. 2) For the following reaction:NH4HS(s)<->NH3(g) + H2S (g) Kc=8.5x10^-3 At any given point the reaction mixture has solid NH4HS, NH3 at 0.166M and H2S at 0.166M. a) Is the reaction at equilibrium? b)Will more of the solid form, or will...
Kp for the reaction CO2(g) + C(s) 2CO(g) is 1.47 at 727°C. Calculate Kc at this temperature
The reaction CO2(g) + C(s)<-->2CO(g) has Kp=5.78 at 1200 K. 1) Calculate the total pressure at equilibrium when 4.73g of CO2 is introduced into a 10.0-L container and heated to 1200 K in the presence of 3.75g of graphite. (I have the answer to this half 1.77 atm) 2) Repeat the calculation of part A in the presence of 0.49g of graphite.
Calculate the value of Kp for the equation C(s) + CO2(g) <--> 2CO(g) Kp = ? Given that at a certain temperature C(s) + 2H2O(g) <--> CO2(g) + 2H2(g) Kp1 = 3.97 H2(g) + CO2(g) <--> H20(g) + CO(g) Kp2 = 0.623
Calculate the value of Kp for the equation C(s)+CO2(g)−⇀↽−2CO(g)Kp=? given that at a certain temperature C(s)+2H2O(g) −⇀↽−CO2(g)+2H2(g)Kp1=3.73H2(g)+CO2(g) −⇀↽−H2O(g)+CO(g)Kp2=0.689
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.
Consider the following reaction: NH4HS(s)⇌NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]= 0.280 M and [H2S]= 0.355 M . What is the value of the equilibrium constant (Kc) at this temperature?
10a 10b. The equilibrium constant, Kp for the following reaction is 0.110 at 298 K. Calculate Kc for this reaction at this temperature. NH4HS(s) NH3+ H2S(g) Ko The equilibrium constant, Kc, for the following reaction is 5.10x10-6 at 548 K. Calculate Kp for this reaction at this temperature NH4CI(sNH)+ HCI(g) Kp
Consider the reaction: NH4HS (s) <--> NH3 (g) + H2S (g). An equilibrium mixture of this reaction at a certain temperature was found to have [NH3] = 0.278 M and [H2S] = 0.355 M. What is the value of the equilibrium constant (Kc) at this temperature? a. 0.126 b. 0.355 c. 0.783 d. 0.0987 e. 0.278
Consider the following reaction: NH4HS(s)⇌NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]= 0.284 M and [H2S]= 0.355 M. You may want to reference (Pages 651 - 653) Section 15.6 while completing this problem. Part A What is the value of the equilibrium constant (Kc) at this temperature?