Consider CO(g) + 2 H2(g) ↔ CH3OH(g) with Kp = 2.26 x 104 at
25ºC. What is ΔGrxn at equilibrium?
0 kJ/mol
13.9 kJ/mol
24.7 kJ/mol
-24.7 kJ/mol
Consider CO(g) + 2 H2(g) ↔ CH3OH(g) with Kp = 2.26 x 104 at 25ºC. What...
Calculate ΔGrxn (in kJ/mol with 1 decimal place) for CH3OH(g) ↔ CO(g) + 2 H2(g) at 25ºC given PCH3OH= 0.855 atm, PCO= 0.125 atm, PH2= 0.357 atm.
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) Kp=2.26×104 at 25 ∘C. Calculate ΔGrxn for the reaction at 25 ∘C under each of the following conditions. Part A: standard conditions Part B: at equalibrium Part C: PCH3OH= 1.5 atm ; PCO=PH2= 1.4×10−2 atm
The reaction below has an equilibrium constant of Kp=2.26×104 at 298 K. CO(g)+2H2(g)⇌CH3OH(g) Part A Calculate Kp for the reaction below. CH3OH(g) CO(g)+2H2(g) Submit My Answers Give Up Part B Reactants will be favored at equilibrium. O Products will be favored at equilibrium. Submit My Answers Give Up Part C Calculate Kp for the reaction below. 를 CO (g) + H2 (g)- CH, OH (g) K=
For the reaction H2(g) + Br2(g) ↔ 2HBr(g) Kp = 3.5 x 104 at 1495 K. What is the value of Kp for the following reaction at 1495 K? 4HBr(g) ↔ 2H2(g) + 2Br2(g) please show work
The reaction below has an equilibrium constant of Kp = 2.26 x 104 at 298 K. CO(g) + 2H2(g) = CH3OH(9) Part A Calculate Kp for the reaction below. CH3OH(g) = CO(g) + 2H2(g) Express your answer to three significant figures. Ky = 4.42-10-5 Submit Previous Answers Completed Part B Calculate K, for the reaction below. CO(g) + H2(g) = = CH3OH(g) Express your answer to three significant figures. ΟΙ ΑΣΦ ? K = Part C Calculate K, for the...
The reaction below has an equilibrium constant of Kp = 2.26 x 104 at 298 K. CO(g) + 2H2(g) = CH3 OH(9) Predict whether reactants or products will be favored at equilibrium in each reaction. Drag the appropriate items to their respective bins. Reset Help Kp = 150 Kp = 1.96 x 10-9 K, = 4.42 x 10 Reactants favored Products favored Submit Request Answer
1) Consider the equilibrium of methanol vapor and the liquid. CH3OH(l)↽−−⇀CH3OH(g) Thermodynamic Table at 25 ∘C Substance ΔHf∘ (kJ/mol) S∘ (J/mol‑K) ΔGf∘ (kJ/mol) CH3OH(l) −239.2 126.8 −166.6 CH3OH(g) −201.0 239.9 −162.3 What is the vapor pressure of the methanol at −30 ∘C? Pvap= atm What is the vapor pressure of the methanol at 40 ∘C? Pvap= 2) Substance ΔG°f(kJ/mol) M2O(s) −8.70 M(s) 0 O2(g) 0 Consider the decomposition of a metal oxide to its elements, where M represents a generic...
step by step please and why What is AGº for this reaction? 1/2 N2(g) + 3/2 H2(g) = NH3(g) Kp = 4.42 104 at 25°C. swer -26.5 kJ.mol-1 -11.5 kJ.mol-1 ered • -2.2 kJ-mol-1 -0.97 kJ-mol-1 Something Else w X
Given the chemical equation, 2 H2O(g) ↔ 2 H2(g) + O2(g) calculate Kp at 1007 K given that the partial pressures of H2O, H2 and O2 at equilibrium are 0.460 bar, 0.055 bar, and 0.045 bar, respectively.
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) The reaction between CO and H2 is carried out at a specific temperature with initial concentrations of CO = 0.26 M and H2 = 0.52 M. At equilibrium, the concentration of CH3OH is 0.11 M. Find the equilibrium constant at this temperature