26) For the equilibrium reaction at 25 °C: Fe(OH),(s) ó Fe" (aq) + 2 ОН (аq), K = 1.61 x 10-14. Calculate [G°in kJ. sp а) —7.87 х 10* d) 2.45 x 103 b) 8.00 x 10' c) 78.7 е) -45.3 f) -2.43 х 103

Be sure to answer all parts. The equilibrium constant K, for the reaction I(g) 5 21(g) is 3.75 x 10 at 726°C. Calculate K, and Kp for the equilibrium 21(g) S1(g) at the same temperature. K.= X 10 %3D (Enter your answer in scientific notation.) Kp = %3D

The formation of ammonia gas from molecular nitrogen and molecular hydrogen gas has the following Kp value. Get the value for the reverse reaction.

Use the References to Consider the following reaction where K, = 2.01 at 500 K: PCI, (g) + Cl,(g)PCI,(g) If the three gases are mixed in a rigid container at 500 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 PCI,(g) is consumed 2. K, will decrease. v 3. A reaction will occur in which PCI, is consumed. | 4. Qis greater than K 5. The reaction is at equilibrium. No further reaction will occur.

A tiny sample of an aqueous solution of two substances R and P is sketched below, as if it was under an imaginary microscope so powerful that individual molecules could be seen. (The water molecules are not shown.) & கக 3 BA R P R and P can interconvert. That is, R can turn into P, and P can turn back into R: K = 2 R(aq)=P(aq) The equilibrium constant K for this equilibrium is 2. Predict the number of R and P molecules in this sample when the interconversion reaches equilibrium.

For the reaction CCl4(g) = C(s) + 2Cl₂(g) Kp = 0.76 at 700 °C. What initial pressure of pure carbon tetrachloride will produce a TOTAL equilibrium pressure of 2.80 atm at 700 °C?

Consider the equilibrium at 25 °C 2 SO3(g)  <==> 2 SO2(g) + O2(g)          Kc= 3.58 x10-3 Suppose that 0.15 mol SO3(g), 0.01 mol SO2(g), and 0.0075 mol O2(g) are placed into a 10.0 L flask at 25 °C. Which of the following statements is true? Q > Kcand will shift from right to left.   Q < Kc and  will shift from right to left.   Q > Kcand will shift from left to right.   Q = Kcand the system is at equilibrium.   Q < Kc and  will shift from left to right.

At 13.7 °C the concentration equilibrium constant K = 2.0 × 10 for a certain reaction. Here are some facts about the reaction: • C The constant pressure molar heat capacity C₁ = 2.49 J-mol K. •If the reaction is run at constant pressure, 147. kJ/mol of heat are released. •If the reaction is run at constant pressure, the volume increases by 13.%. ○ Yes. Using these facts, can you calculate K, at 3.8 °C? x10 No. If you said yes, then enter your answer at right. Round it to 2 significant digits. n If you said no, can you at least decide whether Kat 3.8 °C will be bigger or smaller than K at -13.7 °C? Yes, and K will be bigger. Yes, and K will be smaller. No. x

For this equilibrium system, 2SO3(g) 2 25O2(g) + O2(g), Kc = 0.00407. At equilibrium, you would expect to find %3D relatively more products than reactant. relatively more reactant than products. about comparable amounts of reactant and products. no way to decide.

1. NO2(g) and N₂O4(g) are in a reaction vessel with partial pressures 0.510 bar and 0.800 bar respectively. A,Gº = -2.80 kJ mol-¹. Is this system at equilibrium at 298 K? (a) Yes (b) No