The equilibrium constant in terms of pressures for the reduction of tungsten(IV) oxide to tungsten at 25 °C is Kp = 3.82×10-4, corresponding to the reaction
WO2(s) + 2CO(g) <--> W(s) + 2CO2(g)
If the total pressure of an equilibrium system at 25 °C is 2.82 atm, calculate the partial pressures of CO(g) and CO2(g).
PCO = _____atm
PCO2 = ______atm
The equilibrium constant in terms of pressures for the reduction of tungsten(IV) oxide to tungsten at...
The equilibrium constant in terms of pressures for the reaction SnO2(s) + 2CO(g) Sn(s) + 2CO2(g) at 25 °C is Kp = 0.124. Calculate the reaction quotient Q for each of the following conditions and determine whether solid Sn is consumed or produced as the reaction comes to equilibrium. (A) PCO = 0.249 atm; PCO2 = 0.108 atm; Sn is a) consumed b) produced (B) PCO = 6.34×10-2 atm; PCO2 = 0.174 atm; Sn is a)consumed b) produced
Chemical Equilibrium partial pressure Q1.) I need help with Part 2 on this problem Making CO from CO2 is a potential energy source. The value of Kp for the reaction is is 1.50 at 700.0°C CO2 (g) +C(s) 2CO(g) Q2.) Calculate the equilibrium partial pressure of CO if initially Pco2 1.29 atm and Pco 4.40 atm. Pure graphite is present initially and when equilibrium is achieved 1.94 atm Part 2 (1 pt) O See Hint Calculate the equilibrium partial pressure...
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 in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400 °C is 4.65. (a) If the partial pressure of ammonia is PNH, 0.881 atm and solid ammonium iodide is present, what is the equilibrium partial pressure of hydrogen iodide at 400 °C? PHI atm (b) An excess of solid NH,I is added to a container filled with NH3 at 400 °C and a pressure of 1.17 atm. Calculate the pressures of NH(g) and HI(g)...
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?
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?
Consider the heterogeneous equilibrium process: C(s) + CO2(g) ⇆ 2CO(g) At 700°C, the total pressure of the system is found to be 1.50 atm. If the equilibrium constant (KP) is 1.52, calculate the equilibrium partial pressures of CO and CO2.
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to form SO3 is 0.365 at 1.15×103 K: SO2(g) + O2(g) = 2SO3(g) A sample of SO3 is introduced into an evacuated container at 298 K and allowed to dissociate until its partial pressure reaches an equilibrium value of 0.867 atm. Calculate the equilibrium partial pressures of SO2 and O2 in the container. PSO2 = PO2 =
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.
3a. Determine the equilibrium pressures of all the reactants and products for the equilibrium described below if you start with an initial pressure of carbon dioxide and carbon tetrafluoride each at 0.750 atm with no COF2 present. You can assume that the temperature is constant at 1550K. (12 points) 2COF2(g) CF4(g) + CO2(g) KP = 0.168 at 1550K Initial pressures: PCO2 = PCF4 = 0.750 atm; PCOF2 = 0.000 atm 3b. What is the value of KC for this reaction?...