chem 2 help 22. (5) The equilibrium constant, Kp, equals 6.80 for the isomerization reaction: cis-2-butene...
The equilibrium constant, kp, equals 3.40 at 25°C for the isomerization reaction: cis-2-butene trans-2-butene. If a flask initially contains 5.00 atm of each gas, in what direction will the system shift to reach equilibrium? The system is already at equilibrium. O The system is not at equilibrium and will remain in an unequilibrated state. It will shift right. It will shift left.
The reaction: cis-butene → trans-butene has equilibrium constant K = 2.5 What is the value of Krev for the reverse reaction: trans-butene → cis-butene
chem help
14. At a certain temperature the equilibrium constant, Kc equals 0.11 for the reaction: 2 ICl(g) = 12(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of 12 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask? A) 0.34 M B) 0.14 M. C) 0.27 M D) 0.17 M
The equilibrium constant Kp of the reaction below is 7.69 at 830°C. 2S0,(g) 2S0,(g) +0,(g) 1st attempt ad See Periodic Table See Hint If a vessel at this temperature initially contains pure SO, and if the partial pressure partial pressure of O2 in the flask at equilibrium? of SO3 at equilibrium is 0.100 atm, what is the atm
3. A flask initially containing 0.815 atm of NOBr decomposed to give an equilibrium mixture for the reaction below. If the partial pressure of NO gas at equilibrium was 0.116 atr, then what is the value for the equilibrium constant, Kp, for the reaction? (7 pts) 2 NOBr(g) 2 NO(g) + Br2(1) Kp = 4. Would it be valid to make the simplifying assumption below Why or why not? (3 pts) 0.175- X 0.175 if x = 0.0042
At 800 K, the equilibrium constant, Kp, for the following reaction is 3.2 × 10–7. 2 H2S(g) 2 H2(g) + S2(g) A reaction vessel at 800 K initially contains 3.00 atm of H2S. If the reaction is allowed to equilibrate, what is the equilibrium pressure of S2? Please work the problem out fully and including all work. If you could also explain that would be great!
For the reaction 2A(g) ⇌ B(g) + 2C(s) the equilibrium constant is Kp = 3.6 at a particular temperature. The reaction mixture initially contains 2.0 atm of each gas, A and B, and 10.2 g of C. Choose the statement that is true of the reaction mixture as equilibrium is established at that temperature. A) The reaction will proceed to form more A. B) The outcome cannot be predicted since more data are needed. C) The reaction will proceed to...
1. The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <----> PCl3(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.00 atm at 500 K. PPCl5 = atm PPCl3 = atm PCl2 = atm 2. The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K: NH4I(s) <----> NH3(g) + HI(g) Calculate the equilibrium partial pressure of HI when...
C= C HC c= нен н сн, cis-2-butene irans-2-butene 3. The half-life (t1) of the catalyzed isomerization of cis-2-butene gas to produce trans-2-butene gas, represented above, was measured under various conditions, as shown in the table below. Trial Number Initial Peis-2-bultene (torr) VL T (K) 112 (5) 300. 2.00 350. 100. 2 600 2.00 350. 100. 4.00 350. 100. 300. 2.00 365 50. 300. a. The reaction is first order. Explain how the data in the table are consistent with...
(1). The equilibrium constant, Kp, for the following reaction is 1.80×10-2 at 698K. 2HI(g) =H2(g) + I2(g) If an equilibrium mixture of the three gases in a 15.5 L container at 698K contains HI at a pressure of 0.399 atm and H2 at a pressure of 0.562 atm, the equilibrium partial pressure of I2 is atm. (2). Consider the following reaction: PCl5(g) =PCl3(g) + Cl2(g) If 1.17×10-3 moles of PCl5, 0.217 moles of PCl3, and 0.351 moles of Cl2 are at...