he value of K c for the reaction 2NO 2 (g)  N 2 O 4 (g) is 9.8 at 456 K. What is the value of Kc and K p at this temperature for the reaction 1/2 N 2 O 4 (g)  NO 2 (g)?

3) At 207 °C, Kp = 0.276 for the reactionPCl5(g) ⇌ PCl3(g) + Cl2(g) a. If 0.100 mole of PCl5(g) is placed in an otherwise empty 12.0-L vessel at 207 °C, calculate the partial pressures of PCl5(g), PCl3 (g), and Cl2(g) at equilibrium. b. In another experiment the total pressure of an equilibrium mixture is 2.00 atm at 207 °C. What mass of PCl5 was introduced into an otherwise empty 5.00-L vessel to reach this equilibrium position?

Write the Ke and Kp expressions for the following homogeneous equilibrium reactions: a) CO(g) + -O2(g) = CO2(g) b) 2CO,(g) = O,(g) + 2CO(g) c) N,0(g) = N2(g) + -0,(g)

Suppose a flask contains CH4 at a pressure of 1.80 atm. The reaction below then proceeds to equilibrium.  If KP = 0.0152, what are PH2 and PCH4 at equilibrium?  Set up the ICE problem, then solve it.                  CH4 (g)    =    C(s)     +     2 H2 (g)

At 900 K, the following reaction has Kp = 0.345: 2 SO2(g) + O2(g) ⇋ 2 SO3(g). In an equilibrium mixture, the partial pressure of SO2 and O2 are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3 in the mixture?

Consider the following reaction where K = 7.00×105 at 673 K. NH,I(s)=NH3(g) + HI(g) A reaction mixture was found to contain 5.96×102 moles of NH,I(s), 5.51×103 moles of NH3(g), and 8.37x10-³ moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe, equals| The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

The reaction HCO₂H(g) CO(g) + H₂O(g) has Kp = 1.6 × 106 at 400 °C. What is the value of Kc for this reaction at this temperature? Kc = H

For the reaction PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) Kp = 1.45 × 10⁻⁴ at 160 °C. A 1.00 L vessel at 160 °C is filled with PCl₅(g) at an initial pressure of 3.75 atm and allowed to come to equilibrium. What will be the pressure (in atm) of Cl₂(g) at equilibrium?