Calculate ΔG for this reaction at 25 ∘C under the following
conditions:
PCH3OH= 0.845 atm
PCO= 0.115 atm
PH2= 0.160 atm
CH3OH(g)⇌CO(g)+2H2(g) |
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Calculate ΔG for this reaction at 25 ∘C under the following conditions: PCH3OH= 0.845 atm PCO=...
Consider the following reaction: CH3OH(g)⇌CO(g)+2H2(g) Calculate ΔG for this reaction at 25 ∘C under the following conditions: PCH3OH= 0.840 atm PCO= 0.130 atm PH2= 0.175 atm
Consider the following reaction: CH3OH(g)⇌CO(g)+2H2(g) Calculate ΔG for this reaction at 25 ∘C under the following conditions: PCH3OH= 0.835 atm PCO= 0.135 atm PH2= 0.165 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
73. Consider the reaction: CO(g) + 2H2(g) <--> CH3OH(g) Kp= 2.26X10E4 at 25 C Calculate ΔGorxnfor the reaction at 25C under each of the following conditions: a. standard conditions b. at equilibrium c. PCH3OH= 1.0 atm; PCO= PH2 = 0.010 atm
Calculate ΔG at 25°C for the following reaction: CO(g) + 2H2(g) → CH3OH(l) ΔG°rxn = -2.9x104 J/mol when the carbon monoxide has an initial pressure of 5.0 atm and hydrogen gas of 3.0 atm.
Calculate AG for this reaction at 25 °C under the following conditions : PCH OH 0.850 atm Pco 0.145 atm Pнa = 0.170 atm V ΑΣφ ? kJ AG =
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.
Can someone please help me with these 3 problems and explain it
clear. thank you :)
Consiaer the reaCtIon 75. CO(g)2 H2 (g) = CH3OH(g) K, = 2.26 x 104 at 25 °C Calculate AG,,n for the reaction at 25 °C under each of the following conditions: a. standard conditions b. at equilibrium 1.0 atm; Pco с. Рсн, он = 0.010 atm PH2 Consider the reaction 76. 2(g)Cl2(g)= 2 ICI(g) Kp = 81.9 at 25 °C Calculate AG,,n for the...
A,) ΔG o for the reaction H2(g) + I2(g) ⇌ 2HI(g) is 2.60 kJ/mol at 25°C. Calculate ΔG, and predict the direction in which the reaction is spontaneous. The initial pressures are: PH2 = 3.10 atm PI2 = 1.5 atm PHI 1.75 atm ΔG = kJ/mol b.)The reaction is spontaneous in the forward direction. The reaction is spontaneous in the reverse direction. Cannot be determined.
Calculate ΔG for the formation of ethylene (C2H4) from carbon and hydrogen at 25 ∘C when the partial pressures are 600 atm H2 and 0.30 atm C2H4. 2 C(s)+2H2(g)→C2H4(g) ΔG∘ = 68.1 kJ Is the reaction spontaneous in the forward or the reverse direction?