For the reaction below, determine the equilibrium partial
pressure (in atm) of H2 at 714.10 K if the initial
pressure of HBr is 1.24 atm. Assume that ΔH and ΔS do not vary with
temperature. Report your answer to three significant figures.
LiH (s) + HBr (g) ⇌ LiBr (s) + H2
(g)
ΔHf° (kJ/mol) | S° (J mol-1 K-1) | ||
LiBr | -351.20 | 74.30 | |
H2 | 0.00 | 130.68 | |
LiH | -90.50 | 20.00 | |
HBr | -36.29 | 198.70 |
For the reaction below, determine the equilibrium partial pressure (in atm) of H2 at 714.10 K...
Consider the chemical reaction and thermochemical information and initial partial pressures of the reaction components given below: CH3OH(g) + HBr(g) ⇌ CH3Br(g) + H2O(g) ΔHf° (kJ/mol) S° (J mol-1 K-1) P (atm) CH3Br -35.50 246.40 0.462 H2O -241.83 188.84 0.984 CH3OH -201.50 239.80 5.82 HBr -36.29 198.70 5.22 Determine ΔG (in kJ) for this reaction at 867.29 K. Assume ΔH°f and S° do not vary as a function of temperature. Report your answer to two decimal places in...
For the following reaction: 2Na(s) + 2H2O(l) → 2NaOH(s) + H2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) Na (s) 0.00 51.30 H2O (l) -285.83 69.91 NaOH (s) -425.93 64.46 H2 (g) 0.00 130.68 Calculate ΔG°rx (in kJ) at 391.96 K for this reaction. Assume ΔH°f and S° do not vary as a function of temperature.
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C2H(g)H2(g)2 CH (g) 4 the standard change in Gibbs free energy is AG° -69.0 kJ/mo. What is AG for this reaction at 298 K when the partial 0.400 atm, PH Рс,н, 0.450 atm, and PCH, = 0.600 atm? pressures are kJ/mol AG =
For the following reaction: 2CH4(g) + O2(g) → 2CO(g) + 4H2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CH4 (g) -74.87 188.66 O2 (g) 0.00 205.70 CO (g) -110.53 197.66 H2 (g) 0.00 130.68 Calculate ΔG°rx (in kJ) at 345.31 K for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ). Assume ΔH°f and S° do not vary as a function of temperature.
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N (8) + 3H2(g) + 2NH3(g) the standard change in Gibbs free energy is AGⓇ = -72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.200 atm, PH, = 0.450 atm, and PNH, = 0.750 atm? AG= L kJ/mol AG= kJ/mol
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction the standard change in Gibbs free energy is delta G degree = -72.6 kJ/mol. What is delta G for this reaction at 298 K when the partial pressures are PNO = 0.l00 atm, PO2 = 0.150 atm, and PNO2 = 0.650 atm Number delta G = kJ/mol
Calculate the partial pressure (in atm) of HBr at equilibrium when 3.16 atm of CH3Br and 6.55 atm of H2O react at 1000 K according to the following chemical equation: CH3Br (g) + H2O (g) ⇌ CH3OH (g) + HBr (g) Kp = 6.66×10-2 Report your answer to three significant figures in scientific notation.
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N 2 ( g ) + 3 H 2 ( g ) − ⇀ ↽ − 2 NH 3 ( g ) the standard change in Gibbs free energy is Δ G ° = − 32.8 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are P N 2 = 0.100 atm...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) 2 NO ( g ) + O 2 ( g ) ↽ − − ⇀ 2 NO 2 ( g ) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol Δ G ° = − 72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.300 atm P NO...
For a gascous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction (2NO(g) +0,(8) 2NO,(8) the standard change in Gibbs free energy is AG - -72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are Pro -0.350 atm, Po, -0.500 atm, and Pro, -0.900 atm? 63.96 kJ/mol AG -