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- Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.ntActivity.do?locator assignment-take 40 [Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 182 kJ, and Kc = 7.00x 10-5, at 673 K. NH4I(s)=`NH3(g) + HI(g) When some moles of NH4I(s) are removed from the equilibrium system at constant temperature: The value of Kc The value of Qc Kc. The reaction must Orun in the forward direction to restablish equilibrium. O run in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium. The concentration of NH3 will Submit Answer Previous Without Booting p Retry Entire Group 1 more group attempt remaining SONY WEB OX DISPLA A Other Bookmarks A 4:15 AM 4/30/2022 VGN-NW350F
- For the reaction below, formation salpies at 1 bar and standart entropies are given. Çe te equilibrium constant (Kp) of the reaction at 580 K. X(g) +3 Y,(g) =2XY,(g) For X,(g) AHº,f =0 kJ mol S° = 179 J mol* K For Y(g) AH°f = 0kJ mol* S° = 215 J mol"K** For XY,(g) AH°f = -146 kJ mol" S° = 154 mol K* R = 0.08206 L atm mol-1 K-1 = 8.314 J mol-1 K-1entActivity.do?locator-assignment-take Ikanbewy Tfapies Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 10.4 kJ, and K. = 1.80×10 at 698 K: 2HI(g) H2(g) + I½(g) If the TEMPERATURE on the equilibrium system is suddenly increased: The value of K, A. Increases B. Decreases C. Remains the same The value of Q. A. Is greater than K. B. Is equal to K C. Is less than K. The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of I, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining 50 hp1. The equilibrium constant of the reaction 2 C3H5 (g) = C2H4 (g) + C4H8 (g) is found to fit the expression ln K = - 1.04 - (1088 / T) + (1.51 x 105 / T^2 ) between 300 K and 600 K. Calculate the standard reaction enthalpy and standard reaction entropy at 400 K. [2.77 kJ mol-1 ; -16.5 kJ K-1 mol-1 ]
- 4. In the gas phase reaction 2A + B = 3C + 2D It is found that when1.00 mole A, 2.00 moles B and 1.00 mole D were mixed and allowed to come to equilibrium at 25°C, the resulting mixture 0.9 mole C at a total pressure of 1 bar. Calculate: (i) Mole fraction of each species at equilibrium (ii) Mole fraction equilibrium Kx (iii) Equilibrium K (iv) A,GºA mixture of isobutylene ((CH:)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas-phase thermal decomposition of tert-butyl chloride ((CH:)3CCI) is 3.45 at 500.0 K. (CH:):CCI(g) = (CH:)»CCH:(g) + HCI(g) Based on your ICE table, set up the expression for K for the decomposition of (CH:)»CCI. (CH:):CCI(g) = (CH:).CCH2(g) + HCI(g) 1 Do not combine or simplify terms. K 3.45The below reaction was found to have AH = -406 kJ mol- and AS = 223 J mol-1 K-1. What is AG for this reaction at 118.5 °C? 2Al(s) + 6HCI(aq) – 2AICI;(s) + 3H2(g) Oa. -493 kJ mol-1 Ob. -629 kJ mol-1 Oc. -432 kJ mol-1 Od. -183 kJ mol-1 Oe. -380 kJ mol-1
- es Lx Give Up? Y Hint For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N,(g) + 3 H, (g) =2 NH,(g) the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial %3D pressures are PN, = 0.100 atm, PH, = 0.300 atm, and PNH, = 0.650 atm? %3D %3D kJ/mol AG = TOOLS x10 about us careers privacy policy terms of, use contact us helpthe following thermesdyna mic and partial prassuce data, detormine the Gibbs Energy (AG) for the reaction : Give 2 PeO cg) Clz cq> 2 2 Pe OCI (9) at 298 k in kJ /mol substance AG (KJ/ncol ) P (bar) Pe O cg> - 220.4 0.40 ch (q? Information is missing 0.17 PeOckgs 420.4 0.59(2000″°C given that tựệt° = +1°]\]=d²° a The standard enthalpy of a certain reaction is approximately constant at +125 kJ mol-1 from 800 K up to 1500 K. The standard reaction Gibbs energy is +22 kJ mol-1 at 1120 K. Estimate the temperature at which the equilibrium constant becomes greater than 1.