A reaction occurs in the left-to-right direction until it reaches equilibrium. Which of the following statements is/are completely correct for this reaction? Give some reasoning.    A) At first, ΔSo of reaction > 0 but, when equilibrium is reached, ΔSo = 0. B) At first the reaction is exothermic and it continues until it is thermoneutral (ΔH = 0) C) ΔGo of reaction (which is a constant) remains negative throughout, else no reaction at all would occur. D) At first, the free energy, G > 0, but, when equilibrium is reached, G = 0. E) At first, the free energy change, ΔG < 0, but, when equilibrium is reached, ΔG = 0.

Consider the following general reaction: A(g) ⇌ B(g) Assuming that the ΔGo for this reaction is +50.2 J/mol, what is the equilibrium constant of this reaction at 420 K? (Please provide your answer to 3 significant figures.)

Given the below thermodynamic data, calculate ΔΔH for the reaction CH4 (g) + NH3 (g) ⟶⟶ HCN (g) + 3 H2 (g):    N2 (g) + 3 H2 (g) ⟶⟶ 2 NH3 (g)                                 ΔΔH = -85.6 kJ    C (s) + 2 H2 (g) ⟶⟶ CH4 (g)                                      ΔΔH = -75.2 kJ    H2 (g) + 2 C (s) + N2 (g) ⟶⟶ 2 HCN (g)                  ΔΔH = +271.4 kJ

Find ΔG°rxn for the reaction: N2O(g) + NO2(g)¡ 3 NO(g) Use the following reactions with known ΔG°rxn values:2 NO(g) + O2(g)¡2 NO2(g) ΔG°rxn = -71.2 kJN2(g) + O2(g)¡2 NO(g) ΔG°rxn = +175.2 kJ2 N2O(g)¡2 N2(g) + O2(g) ΔG°rxn = -207.4 kJ

Consider the Gibbs free energy change for the conversion of glucose to fructose that occurs during the metabolism of sugar (∆GRXN = +2.1 kJ) What is the value of the equilibrium constant (Keq) when the conversion takes place at 24.9 °C?

17. The thermochemical equation for the reaction of F2 and water is as follows. AH = -270 kJ F2(g) + 2 H2O (liq)=HF (aq) + O2 (g) Given a system that is initially at equilibrium, which of the following actions cause the reaction to proceed to the right? a) adding O2(g) b) decreasing the temperature c) adding a catalyst d) decreasing the volume of the reaction chamber e) none of the above

Use the thermodynamic data provided below to determine the ΔGº for the reaction. 1A(s) + 4B(g) -> 1C(s) + 2D(g) Given the following: ΔGf° = -96.0 kJ mol-1 for substance A (s) ΔGfº = 254.0 kJ mol-1 for substance B (g) ΔGfº = 59.0 kJ mol-1 for substance C (s) ΔGfº= 248.0 kJ mol-1 for substance D (g) Provide your answer with final units of kJ and to one decimal place.

[Review Topics] [References) Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° =-10.4 kJ/mol, and K. = 55.6 , at 698 K. H2 (g) + I2 (g)=2 HI (g) When 0.26 moles of HI (g) are added to the equilibrium system at constant temperature: The value of K. The value of Q. v Ke The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. O remain the same. It is already at equilibrium. The concentration of I, will Submit Answer Retry Entire Group 9 more group attempts remaining (Previ ins prt sc delete fg f10 f12

Calculate the temperature at which the reaction below will be at equilibrium, then explain how this temperature can affect the spontaneity, meaning how using higher or lower than this temp can affect the value of delta G.   Given.      Br2(l) → Br2 (g),  ΔH = 31.0 kj/mol ΔS = 92.9 j/mol

11. What is the ΔHº-value for the dissolution of NaOH (s) to yield 1.00... m NaOH (aq), given:      Na (s) + 1/2 O2 (g) + 1/2 H2 (g) → NaOH (s)              ΔHfº = -425.9 kJ/mol   Na (s) + 1/2 O2 (g) + 1/2 H2 (g) → NaOH (aq, 1 m)    ΔHfº = -469.2 kJ/mol     Multiple Choice   -895.1 kJ/mol   -43.3 kJ/mol   +1.102 kJ/mol   +43.3 kJ/mol   +895.1 kJ/mol