For the reaction N2O4(g) = 2 NO2(g), the pressure equilibrium constant Kp is 0.144 at 25oC and 0.321 at 35oC. Find delta G^o, delta H^o and delta S^o at 25oC.

The growth of baker's yeast (Saccharomyces cerevisiae) on glucose under anaerobic conditions can be described by the following equation:C6H12O6 + β NH3 → 0.59 CH1.74N0.2O0.45 + 0.43 C3H8O3 + 1.54 CO2 + 1.3 C2H5OH + 0.036 H2O a) Determine the value of the biomass yield coefficient YX/Sb) Determine the values of the yield coefficients in products YEtOH/S and Yglycerol/Sc) Calculate the value of the coefficient β

For the gas-phase reaction of water shown below, A,G° = 118.08 kj mol"1 when T= 2300 K. H,0(g) = H2(g) +;0;(g) a) What is the value of the equilibrium constant at 2300 K? b) What is Kp (the equilibrium expression in terms of partial pressures) for this reaction? c) What is the degree of dissociation of H20 at 2300 K and 1.00 bar? Recall that the degree of dissociation is defined as a = (no - neoVng- %3D

Consider the reaction H2CO(g) + 02(g) Co2(g) + H20(1) for which AH° = -563.3 kJ and AS° = -140.5 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 2.085 moles of H,CO(g) react under standard conditions at 298.15 K. ASuniverse = J/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'. Submit Answer

QUESTION 8 Regarding the following reaction CO2 (g)+H2 (g)→→CO(g)+H₂O (g) ArH=-41.2kJ/mol Using Le Chatelier's principle to predict (a) to which direction the equilibrium shifts when pressure is decreased. Enter R for reactants, P for products and N for Neither: Direction= ; (b) to which direction the equilibrium shifts when temperature is reduced. Enter R for reactants, P for products and N for Neither: Direction=

a. Consider the endothermic reaction: 2 HgO (s) → 2 Hg (l) + O2 (g),  ΔH = 181.66 kJ/mol b. Consider the reaction: 2 C (graphite) + O2 (g) → 2 CO (g),  ΔH = –221 kJ/mol c. Consider the endothermic reaction: CdSO4 (s) → Cd2+ (aq) + SO42− (aq),    > 0 This reaction is nonspontaneous spontaneous at all temperatures spontaneous at low temperatures spontaneous at high temperatures

Using enthalpies of formation, calculate AHrxn for the reaction: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(()

Nitrosyl bromide, NOBr, decomposes according to the equationNOBr(g) → NO(g) + 1/2 Br₂(g)where ∆G˚ at 4.0e+02 ˚C is 9.83 kJ. What is the value of the equilibrium constant at 4.0e+02˚C?

C) A sample of Al (2.8 g) reacts with a sample of Cl (4.15 g) according to equation below: 2Al(s) + 3CI2 (g) → 2AIC33(s) What is the theoretical yield of AIC13 in this reaction? The mass number for Al is 27 while for Cl is 35

Calculate the reaction enthalpy for the reaction below: 2 C(s) + D (g) →→→2 A (s) +2B (s) given the following information X (s) + D (g) →→→ A (s) Y(g) +B(s)→→→ Z (g) X (s) +Z (g) →→→ C(s) +Y(g) AH, : AH, = ? kJ AH₁ = -263.0 kJ AH₂ = -75.0 kJ AH3 = -455.0 kJ kJ