3CH4(g)→C3H8(g)+2H2(g)
Calculate ΔG at 298 K if the reaction mixture consists of 41 atm of CH4, 0.013 atm of C3H8, and 2.0×10−2 atm of H2.
given
3CH4(g)→C3H8(g) + 2H2(g)
PC3H8= 0.013 atm
PH2 = 2.0×10−2 atm
PCH4 = 41 atm
we know that
ΔG = ΔG0 + RTlnQ
lets calculate ΔG0of the reaction
ΔG0rxn = ΔG0 f(products) - ΔG0 f(reactants)
= (ΔG0 f(C3H8(g)) + 2*ΔG0 f(H2(g)) ) – (3*ΔG0 f(CH4(g)))
Now
ΔG0 f(C3H8(g)) = -24.40 kJ/mol
ΔG0 f(CH4(g)) = -50.80 kJ/mol
ΔG0 f(H2(g)) = 0 kJ/mol
ΔG0rxn = (-24.40 kJ/mol – 2*0) – (3*-50.80 kJ/mol)
= -24.40 kJ/mol + 152.40 kJ/mol
= 128 kJ/mol
So
ΔG0 = 128 kJ/mol
Q = Pproducts/Preactants
= (PC3H8) * (PH2)2 / (PCH4)3
= (0.013)* (2.0×10−2)2 / 413
= 0.013 * 4*10-4 / 68921
= 7.5 * 10-11
ln(Q) = -23.3
now
ΔG = ΔG0 + RTlnQ
= 128 kJ/mol + (8.314 J/mol K * 298 K * -23.3)
= 128 kJ/mol – 57.727 kJ/mol
= 70 kJ/mol
3CH4(g)→C3H8(g)+2H2(g) Calculate ΔG at 298 K if the reaction mixture consists of 41 atm of CH4,...
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g) ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is ________. -3.86 × 103 -1.8 -7.25 × 103 -104.5 -40.5
Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K Calculate the following quantities. ΔSsys=ΔSsys J/K ΔSsurr= J/K ΔSuniv= J/K
Consider the following reaction at 298 K.C(graphite) + 2H2(g)→ CH4(g) ΔH°=-74.6 kJ
The reaction C(s)+2H2(g)⇌CH4(g) has Kp=0.263 at 1000. K. Calculate the total pressure at equilibrium when 5.759 g of H2 and 22.94 g of C(s) are placed in a 9.88 L flask and heated to 1000. K. Ptotal= ? atm Calculate the total pressure when 5.759 g of H2 and 8.755 g of C(s) are placed in a 9.88 L flask and heated to 1000. K. Ptotal= ? atm
Use the following data to calculate the value of ΔG°rxn at 298 K for the reaction described by the given chemical equation. Include the units. Compound S°f (J/molK) DH°f (kJ/mol) CO (g) 197.7 –110.5 H2 (g) 130.7 0 CH4 (g) 186.3 –74.6 H2O (g) 188.8 –241.8 CO (g) + 3H2 (g) → CH4 (g) + H2O (g) I got -141.9 KJ/mol, but i think the units are wrong and I don't know why.
Consider the reaction at 298 K. C(graphite)+2 H 2 (g)⟶ CH 4 (g)Δ?°=−74.6 kJ C(graphite)+2H2(g)⟶CH4(g)ΔH°=−74.6 kJ Calculate the quantities. Delta Ssys=_______ J/K Delata Ssurr =_______ J/K
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.
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
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=