Consider this reaction at 298 K:
H2 (g) + I2 (g) ⇌ 2 HI(g)
Calculate ΔGrxn under the following conditions:
PH2 (g) = 0.161
atm
PI2 (g) = 0.186 atm
PHI(g) = 0.307 atm
Consider this reaction at 298 K: H2 (g) + I2 (g) ⇌ 2 HI(g) Calculate ΔGrxn...
Consider the following reaction: I2(g)+Cl2(g) ⇌ 2ICl(g) Kp= 81.9 at 25 ∘ C. Calculate ΔGrxn for the reaction at 25 ∘ C under each of the following conditions. Part A. Standard conditions Part B. At equilibrium Part C. PICl= 2.59 atm PI2= 0.322 atm PCl2= 0.221 atm
Consider the following reaction: I2(g)+Cl2(g) ⇌ 2ICl(g) Kp= 81.9 at 25 ∘ C. Calculate ΔGrxn for the reaction at 25 ∘ C under each of the following conditions. PICl= 2.58 atm PI2= 0.322 atm PCl2= 0.214 atm Express your answer using one significant figure.
Consider the following reaction: I2(g)+Cl2(g) ⇌ 2ICl(g) Kp= 81.9 at 25 ∘ C. Calculate ΔGrxn for the reaction at 25 ∘ C under each of the following conditions. PICl= 2.58 atm ; PI2= 0.324 atm ; PCl2= 0.221 atm . Express your answer using one significant figure.
. Consider the reaction: H2(g) + I2(g) ? 2HI(g) A reaction mixture at equilibrium at 175 K contains PH2 = 0.958 , PI2 = 0.877 , and PHI= 0.020 . A second mixture not equilibrium, but at the same temperature,contains PH2 = PI2 = 0.621 , and PHI = 0.101 . a) For the second mixture, calculate Q. b) Determine whether the reaction in the second mixture will shift right or shift left.c) Construct an ICE table. Keep in mind your...
Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ P(O2) = 0.41 atm, P(O3) = 5.2 atm
Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ P(O2) = 0.20 atm, P(O3) = 0.038 atm kj = ?
The equilibrium constant for the following reaction is 50.5 at 448 oC. H2(g) + I2(g) ⇌ 2 HI(g) a. Find DGorxn at 448 oC. (This is the change in free energy when the partial pressure of each gas is 1 atm and the T is 448 oC.) b. What is DGrxn when T = 448 oC and PH2 = 1 atm, PI2 = 0.1 atm, PHI = 0.1 atm? c. Is the forward reaction spontaneous...
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.
For the reaction H2 S(g) + I2 (s) ⇌ S(s) + 2 HI(g) Kp = 1.33×10–5 at 333 K. What will be the total pressure of the gases above an equilibrium mixture if, at equilibrium, PHI = 0.010 × PH2 S? The answer is 0.134 atm. Please include work and explanation! Thank you :-)
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