front 1 Enthalpy is favored when... | back 1 H < 0 |
front 2 Entropy is favored when... | back 2 S > 0 |
front 3 When the S universe is positive then the reaction is ____ favored | back 3 product |
front 4 2NO(g) + 2H2(g) N2(g) + 2H2O(l) for which Ho = -752.2 kJ and So = -351.6 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 2.175 moles of NO(g) react under standard conditions at 298.15 K. (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored choose 'reactant favored' | back 4 2361 product enthalpy |
front 5 If a lower temp is required to reach the same vapor pressure as another molecule, then the first molecule have _____ IMF | back 5 weaker |
front 6 For silicon, Si, the heat of fusion at its normal melting point of 1410oC is 46.4 kJ/mol. The entropy change when 2.23 moles of liquid Si freezes at 1410oC, 1 atm is | back 6 -61.5 |
front 7 equilibrium phase change formula | back 7 Sphase = Hphase/Tphase |
front 8 The molar solubility of manganese(II) hydroxide in a 0.159 M manganese(II) nitrate solution is | back 8 2.7E-7 |
front 9 Ksp equation | back 9 [x][y] |
front 10 If a chemical reaction occurs in a direction that has a positive change in entropy then | back 10 disorder increases |
front 11 If H < 0 and S > 0 then... | back 11 always spontaneous |
front 12 If H < 0 and S < 0 then... | back 12 spontaneous at low temp |
front 13 If H > 0 and S > 0 then... | back 13 spontaneous at high temp |
front 14 If H > 0 and S < 0 then... | back 14 never spontaneous |
front 15 trend of molecule size, attractive forces, and entropies | back 15 As a molecule gets bigger, the attractive forces decrease As the attractive forces decrease, the entropies increase As the molecule gets bigger, entropies increase |
front 16 how to calculate new pressure at new volume | back 16 P2 = (V2/V1) x P1 |
front 17 vapor will condense if... | back 17 it is more than the given pressure ex: P > 100mm Hg |
front 18 From the following vapor pressure data for pentane, an estimate of the molar heat of vaporization of C5H12 is P, mm Hg T, Kelvins | back 18 27.3 |
front 19 Consider the insoluble compound silver hydroxide, AgOH. The silver ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of AgOH(s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Ag(NH3)2+, Kf = 1.6E+7 | back 19 AgOH(s) + 2NH3(aq) --> Ag(NH3)2+(aq) + OH-(aq) 0.32 (knet = Ksp x Kf) |
front 20 processes that release energy & the phase changes associated | back 20 gas --> liquid: condensation gas --> solid: deposition liquid --> solid: freezing |
front 21 A student determines the value of the equilibrium constant to be 2.57E-25 for the following reaction. CH4(g) + H2O(g) 3H2(g) + CO(g) Based on this value of Keq: Go for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 2.43 moles of CH4(g) at standard conditions at 298K | back 21 greater 341 |
front 22 Calculate ΔrG° for the reaction below at 25.0 °C | back 22 –320.6 kJ/mol-rxn |
front 23 The standard free energy change associated with the dissolution of ammonium nitrate in water is -13.0 kJ/mol at 356 K. NH4NO3(s) NH4NO3(aq) What is the equilibrium constant for the reaction? | back 23 81 |
front 24 The solubility of CaCrO4 is measured and found to be 4.04 g/L. Use this information to calculate a Ksp value for calcium chromate | back 24 6.7E-4 |
front 25 Calculate the solubility of copper(II) sulfide, CuS in units of grams per liter. Ksp(CuS) = 7.9E-37 | back 25 8.5E-17 |