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.
∆G is gibbs free energy & ∆G° is gibbs free Energy at standard state Condition.
Kp is equilibrium constant, when partial pressure is taken into consideration. It is written as the ratio of product of partial pressure of product to the product of partial pressure of reactant.
Partial pressure of CH3OH is taken as 1 as it is pure liquid so it will not exert any partial pressure.
Calculate ΔG at 25°C for the following reaction: CO(g) + 2H2(g) → CH3OH(l) ΔG°rxn = -2.9x104...
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
Carbon monoxide gas reacts with hydrogen gas to form methanol via the following reaction: CO(g)+2H2(g)→CH3OH(g) A 1.70 L reaction vessel, initially at 305 K, contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 355 mmHg . Identify the limiting reactant and determine the theoretical yield of methanol in grams
1.Carbon monoxide gas reacts with hydrogen gas to form methanol via the following reaction: CO(g)+2H2(g)→CH3OH(g)CO(g)+2H2(g)→CH3OH(g) A 1.65 LL reaction vessel, initially at 305 KK, contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 395 mmHg. Identify the limiting reactant and determine the theoretical yield of methanol in grams. Express your answer with the appropriate units. 2. What is the pressure in a 12.0-LL cylinder filled with 39.5 g of oxygen...
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 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)
Delta G f(CO)= -137.3 kJ/molDelta G f(CH3OH)= -166.3 kJ/molDelta H f(CO)= -110.5 kJ/molDelta H f(CH3OH)= -238.7 kJ/molS(CO)= 197.9 J/K molS(CH3OH)= 126.8 J/K molCalculate Delta G at 25 Degrees Celcius.
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?
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.17 −L flask at a certain temperature contains 27.0 g CO and 2.35 g H2. At equilibrium, the flask contains 8.67 g CH3OH. Calculate the equilibrium constant (Kc) for the reaction at this temperature. Kc=?