4. IBr decomposes according to the reaction at 150 C: 2 IBr (g) = I2 (g) + Br2 (g) If IBr is placed in a container at an initial pressure of 5.0 atm, what will be its %3D equilibrium pressure at 150°C? Kp = 8.3 x 10-3

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At 1000 K, a sample of pure NO₂ gas decomposes: 2 2NO₂(g) = 2NO(g) + O₂(g) The equilibrium constant Kp, is 158. Analysis shows that the partial pressure of O₂ is 0.41 atm at equilibrium. Part 1 of 2 What is the pressure of NO? Be sure your answer has the correct number of significant digits. Part 2 of 2 atm x10 atm X What is the pressure of NO₂? Be sure your answer has the correct number of significant digits. Ś x10

The reaction H2(g) + I2(g)  2HI(g) has Kp = 45.9 at 763 K. A particular equilibrium mixture at 763 K contains HI at a pressure of 3.01 atm and H2 at a pressure of 2.62 atm. Calculate the equilibrium pressure of I2(g) in this mixture.

At 1560 oC the equilibrium constant for the reaction: 2 IBr(g)  I2(g) + Br2(g) is KP = 0.846. If the initial pressure of IBr is 0.00674 atm, what are the equilibrium partial pressures of IBr, I2, and Br2?p(IBr) =  p(I2) =  p(Br2) =

An empty steel container is filled with 0.840 atm of A and 0.840 atm of B. The system is allowed to reach equilibrium according to the reaction below. If Kp = 340 for this reaction, what is the equilibrium partial pressure of C? A (g) + B (g) = C (g)

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)

Some quantity of NOBr is added to an otherwise empty flask. The reaction: 2 NOBr (g) ⇄ 2 NO (g) + Br2 (g) takes place at a particular temperature for which KP  is 3.5 x 10-5. Assuming an equilibrium pressure of NOBr = 2.46atm, what is the equilibrium pressure of NO?

The equilibrium constant Kp for the reaction PC15(g) = PC13(g) + Cl₂(g) is 1.05 at 250°C. The reaction starts with a mixture of PC15, PC13, and Cl₂ at pressures 0.177 atm, 0.233 atm, and 0.161 atm, respectively, at 250°C. When the mixture comes to equilibrium at that temperature, which pressure(s) will have decreased? Cl₂ PC13 PC15

At a particular temperature, the reaction below has a K value of 1.03 x 10-2. If [SO3] = 0.97M, [SO2] = 1.4 x 10-1M, and [O2] = 0.83M, determine if the reaction is at equilibrium, needs to shift right to reach equilibrium, or if it needs to shift left to reach equilibrium. 2 SO3(g) <---> 2 SO2(g) + O2(g) a. Q less than K, shift right b. Q greater than K, shift left c. Q less than K, shift left d. Q greater than K, shift right  e. at equilibrium