The equilibrium constant Kp for the reaction C(s)+H2O(g)⇌CO(g)+H2(g) is 2.44 at 1000 K. What are the equilibrium partial pressures of H2O, CO, and H2 if the initial partial pressures are PCO=1.15 atm, and PH2= 1.45 atm?
Part A
What is the equilibrium partial pressure of H2O?
Part B
What is the equilibrium partial pressure of CO?
Part C
What is the equilibrium partial pressure of H2?
The equilibrium constant Kp for the reaction C(s)+H2O(g)⇌CO(g)+H2(g) is 2.44 at 1000 K. What are the...
The equilibrium constant Kp for the reaction C(s)+H2O(g)⇌CO(g)+H2(g) is 2.44 at 1000 K. What are the equilibrium partial pressures of H2O, CO, and H2 if the initial partial pressures are PCO= 1.30 atm, and PH2= 1.40 atm? Part A What is the equilibrium partial pressure of H2O? What is the equilibrium partial pressure of CO? What is the equilibrium partial pressure of CO?
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...
Under certain conditions, the reaction H2O(g) + C(s)=CO(g) + H2(g) is at equilibrium, and the Kp is 5. The partial pressure for H2O is 1.5 atm, for CO is 3.0 atm. What is the partial pressure of Hy in atm?
Be sure to answer all parts. The equilibrium constant (Kp) for the reaction below is 4.40 at 2000. K. H2(g) + CO2(g) ⇌ H2O(g) + CO(g) Calculate Δ G o for the reaction. kJ/mol Calculate Δ G for the reaction when the partial pressures are PH2 = 0.22 atm, PCO2 = 0.83 atm, PH2O = 0.66 atm, and PCO = 1.12 atm.
The equilibrium constant (Kp) for the reaction below is 4.40 at 2000. K. 0 Calculate AG for the reaction 24.64 kJ/mol Calculate AG for the reaction when the partial pressures are PH, 0.28 atm, Pco,0.75 atm, H2O = 0.65 atm, and CO*. Pco-1.16 atm.
The equilibrium constant (Kp) for the reaction below is 4.40 at 2000. K. 0 Calculate AG for the reaction 24.64 kJ/mol Calculate AG for the reaction when the partial pressures are PH, 0.28 atm, Pco,0.75 atm,...
At 6 oC the equilibrium constant for the
reaction:
2 HI(g) H2(g) + I2(g)
is KP = 2.66e-11. If the initial pressure of HI is
0.00837 atm, what are the equilibrium partial pressures of HI,
H2, and I2?
We were unable to transcribe this imageAt 6 °C the equilibrium constant for the reaction: 2 HI(g) = H2(g) + 12(g) is Kp = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI,...
At 1000 K, Kp = 19.9 for the following reaction: Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g) What are the equilibrium partial pressures of CO and CO2 if CO is the only gas present initially, at a partial pressure of 0.982 atm ?
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium partial pressures of all species when H2 and I2, each at an intitial partial pressure of 1.65 atm, are introduced into an evacuated vessel at 698 K.
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium partial pressures of all species when CO and Cl2, each at an intitial partial pressure of 1.70 atm, are introduced into an evacuated vessel at 600 K. PCO = atm PCl2 = atm PCOCl2 = atm B. The equilibrium constant, Kc, for the following reaction is 2.90×10-2 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) Calculate Kc at this temperature for...
At 1000 K, Kp = 19.9 for the reaction Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g). What are the equilibrium partial pressures of CO and CO2 if CO is the only gas present initially, at a partial pressure of 0.986 atm ? Enter your answers numerically separated by a comma.