Consider the reaction: 2NO2(g) N204(g) for which (at 25\deg C) AH\deg = -56.8 kJ and AS\deg = -175 J/ K. Mark the statements which are correct. (Select all that apply.) Kp for this reaction will increase as T is increased. This is an exothermic reaction as written. AG\ deg for this reaction is negative. Kp for this reaction is less than 1.00.

Given the information A+ B 2D AH = -759.3 kJ AS = 368.0 J/K C→ D AH° = 432.0 kJ AS = -126.O J/K calculate AG at 298 K for the reaction A +B 2C AG = 1808.06 Incorrect Activate Windo Go to Settings to actro help terms of use contact us careers privacy policy about us

[Review Topilos] 10Refaeiyas 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. = 55.6 , at 698 K: H2 (g) + I2 (g)= 2 HI (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 Prev 50

48 Use data to compute ΔG° at 57.0°C for the following reaction. 2ClO2−(aq) + O2(g) → 2ClO3−(aq) ΔH°f (ClO2−(aq)) = -67 kJ mol-1ΔH°f (ClO3−(aq)) = -104 kJ mol-1ΔS° (ClO2−(aq)) = 101 J mol-1 K-1ΔS° (O2(g)) = 205.152 J mol-1 K-1ΔS° (ClO3−(aq)) = 162 J mol-1 K-1ΔG°f (ClO2−(aq)) = 17 kJ mol-1ΔG°f (ClO3−(aq)) = -3 kJ mol-1