At 333 K, this reaction has a K, value of 0.0709. 2 X(g) +3 Y(g) Z(g) Calculate K₂ at 333 K. Note that the pressure is in units of atmosphere (atm). Kp = 3.47 X10-6

At 429 K, this reaction has a K. value of 0.0407. X(g) + 2 Y(g) = Z(g) Calculate Kp at 429 K. Note that the pressure is in units of atmosphere (atm). Kp =

Consider the following chemical equilibrium: C(s) + 2 H₂ (g) ⇒ CH₂(g) Now write an equation below that shows how to calculate K from K for this reaction at an absolute temperature T. You can assume I is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K -0 X 00

The reaction C(s) + 2 H₂(g) = CH₂(g) has Kp = 0.263 at 1000. K. Calculate the total pressure at equilibrium when 4.305 g of H₂ and 22.06 g of C(s) are placed in a 9.08 L flask and heated to 1000. K. Ptotal = Calculate the total pressure when 4.305 g of H₂ and 7.404 g of C(s) are placed in a 9.08 L flask and heated to 1000. K. Ptotal = atm atm

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)

An experimenter places the following concentrations of gases in a closed container: NOBI]=0.245 M, [NO] = 3.29 x 10 M, Br2] = 2.02 x 10- M These %3D gases then react: 2NOB1(g) 2NO(g) + Br2 (g) 4. At the temperature of the reaction, the equilibrium constant K, is 5.85 x 10 * Calculate the reaction quotient, Q, from the initial concentrations and determine whether the concentration of NOBR increases or decreases as the reaction approaches equilibrium. Q.= %D The concentration of NOBR

Consider the reaction: 2 H2S (g) ⇋ 2 H2 (g) + S2 (g) Kp = 2.4 x 10 -4 at 1073 K If the initial pressure of hydrogen sulfide is 755 torr, what will be the equilibrium partial pressure of each gas?

At 487 K, this reaction has a Ke value of 0.0463. 2 X(g) + 3 Y(g) = 2Z(g) Calculate Kp at 487 K. Note that the pressure is in units of atmosphere (atm). Kp =

For the reaction 2 A(g) = B(g) + 3 C(g), we begin with only pure A(g) and the total pressure is 8.00 atm. We attain equilibrium. At equilibrium, the total pressure is 12.00 atm. What is the value of ∆G◦ for this reaction? The temperature is 25.0 ◦C throughout.

Consider the following reaction where K, = 6.50x10-3 at 298 K. 2NOBR(g) =2NO(g) + Br2(g) A reaction mixture was found to contain 8.79x10-2 moles of NOBR(g), 2.03x10-2 moles of NO(g), and 4.53x10 2 moles of Bro(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, Qc, 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.