Incorrect Question 1 0/1 pts At 699 K, AGⓇ = -23.25 kJ for the reaction H2...
At 699 K, AG° = -23.25 kJ for the reaction H2(g) + 12(g) = 2 HI(g). Calculate AG for this reaction if the reagents are both supplied at 10.0 atm pressure and the product HI is at 1.00 atm pressure. Select one: O a. -36.6 kj O b. -50.0 kj O C. -3.5 kg O d. +50.0 kJ o e. +36.6 kJ
15. At 699 K AG° = -23.25 kJ for the reaction H2g) + 12(a)= 2Hg). Calculate AS this reaction if the reagents are both supplied at 10.0 atm pressure and the pro is at 1.94 atm pressure A) -19.1 kJ B) 19.1 kJ C) 42 kJ D) 42 3 kJ E) 42 3 kJ
() Calculate AGⓇ for the following reaction at 298 K. The AGP values are 0 kJ/mol for C12(e) -325 kJ/mol for Cisce), and -286 kJ/mol for PC13(e). PC1518) PC3(8) + Cl2(g) (b) Calculate AG at 298 K for the reaction if the partial pressures are PC120,40 atm, PPC13 -0.27 atm, and PPCi5 -0.0029 atm.
ΔGf°(I2(g)) = 19 kJ/mol 7. For the reaction H2(g) +12(g) = 2HI(g) K = 50.0 at 721 K (a) What is AG at 721 K? (b) What is Kat 25 °C? (AG HI(g) = +1.7 kJ/mol)
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 the reaction CO(g) + H2O(1)—*CO2(g) + H2(g) AH° = 2.8 kJ and AS° = 76.8 J/K The standard free energy change for the reaction of 2.33 moles of CO(g) at 288 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 288 K. Assume that AH° and ASº are independent of temperature. Submit Answer Retry Entire Group 9 more group attempts remaining For the reaction 2 NO(g) + O2(g) → 2 NO2(g) AG°...
(10 pts) Hydrogen iodide can decompose into hydrogen and iodine gases. K for the reaction is 0.016. If 0.148 atm of HI(g) is sealed in a flask, what is the pressure of each gas when equilibrium is established? 2HI(g) = H2(g) + 12(g) K = 0.016
Find AG (in kJ mol-1 to one decimal place) for the following reaction at 198.15 K when Phi= 2.0 atm, Piz=5.0 atm, and PH2=3.0 atm. H2(g) +12(8) —HI(g)
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction N2(g) + 3 H2(g) = 2 NH3(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 bar, Ph, = 0.150 bar, and PnHz = 0.800 bar. kJ AG = mol