Free Online Survey... demia... [References] Use the References to access important values if needed for this question. Consider the following reaction where Kp = 0.160 at 298 K. 2NOBr(g) 2NO(g) + Br₂(g) If the three gases are mixed in a rigid container at 298 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: 1. A reaction will occur in which NOBr(g) is produced. 2. K, will increase. 3. A reaction will occur in which NO is produced. Submit Answer 4. Qp is greater than Kp. 5. The reaction is at equilibrium. No further reaction will occur. Retry Entire Group 8 more group attempts remaining

The below reaction was found to have AH = -3606 kJ mol-1 and AS = 33 J mol- K-1. What is AG for this reaction at 100.2 °C? 90,(g) + 2CH;CHCH,(g) – 6CO,(g) + 6H2O(g) Oa. -3618 kJ mol-1 Ob. -3609 kJ mol-1 Oc. -15927 kJ mol-1 Od. -3573 kJ mol-1 Oe. -3594 kJ mol-1

For the reaction 2CH,(g) =C,H2(g) + 3H2(g) Ke = 0.155 at 1611 °C. What is K, for the reaction at this temperature? Express your answer numerically. • View Available Hint(s) ? Kp =

2H20(g) + 3N2(g) 2 2N20(g) + N2H4(g) If K, for the above reaction is 781.8 at 200.9 K, what is Kp for the same reaction? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 12.3 and 120. and -123)

Question 15 of 16 Submit Consider the reaction below: 2 SO3(g) =2 SO2(g) + O2(g) The Kp is 1.81 × 10-5 at 350.0°C. Calculate Kc at the same temperature. (R = 0.08314 L·bar/ mol · K.) 1 2 3 4 C 7 8 9 +/- х 100 Tap here or pull up for additional resources LO

For the equilibrium reaction.   2IBr (g) I2 (g) + Br2 (g) Kc=.0085.  If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components.   Consider the decomposition reaction at 555 K   4POCl3 (g)    P4  (g) + 2O2  (g) + 6Cl2  (g)   If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm.  Find Kp and Kc.

In the gas-phase reaction A + B=C+ 2 D, it was found that, when 2.00 mol A, 1.00 mol B and 3.00 mol D were mixed and allowed to come to equilibrium at 25°C, the resulting mixture contained 0.79 mol C at a total pressure of 1.00 bar. Calculate Kp. [.960]

Consider the following reaction where K, = 9.52×10-2 at 350 K: %3D CH4(g) + CC14(g) 2CH2C1½(g) If the three gases are mixed in a rigid container at 350 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: • 1. A reaction will occur in which CH,Cl2(g) is consumed. v 2. K, will increase. • 3. A reaction will occur in which CH, is consumed. • 4. Q is less than K. v 5. The reaction is at equilibrium. No further reaction will occur.

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Consider the following system at equilibrium where K. = 34.5 and AH° = -198 kJ/mol at 1150 K. 2 So, (g) + 02 (g) =2 S03 (g) The production of S03 (g) is favored by: Indicate True (T) or False (F) for each of the following: ]1. decreasing the temperature. v 2. increasing the pressure (by changing the volume). | 3. decreasing the volume. 4. removing SO3 . 5. removing O2 -