Consider the gas phase reaction 302(g) 203(g) (a) At 298K and a total pressure of 1...
Consider the gas phase reaction 302(g) = 203(g). (a) At 298K and a total pressure of 1 atm, what are the partial pressures at equilibrium? (b) What about at 398K and a total pressure of 1 atm?
show your work please... 31. For the reaction: 302(g) 203(g); at equilibrium 0.80g of O2 and 0.24g of Oz was found at 0.20 atm pressure. Calculate the equilibrium constant, Kp. A. 0.50+ B. 0.224 C. 0.045 D. 2.0-
9.3 Consider the gas phase reaction: PCI3(g) Cl2(g) PCI5(g) at equilibrium at 400 K and 1 atm total pressure. The closed system is initially charged with 1 mole of PCI3 and 2 moles of Cl2 The standard free energy change of this reaction is -3.53 kJ/mole. What is the mole fraction of PCI5 at equilibrium?
7. (a) If the partial pressure of each component is 1 atm, and the temperature is 298K, which way does the reaction N204(g) + 2N02(g) go - to the right or to the left? (b) If the system comes to equilibrium at 298K under a total pressure of 1 atm, what will be the partial pressures of each reagent? (c) And at a temperature of 380K?
4. Consider the reaction: 2 NO(g) + Br2 (g) 2 NOB (g) Kp = 31.8 at 302 K a) If the initial partial pressures are Pro = 108 torr, Per; = 126 torr, ProBr = 275 torr, find Qp and determine which direction the reaction proceeds in to reach equilibrium. 139.17 b) When a mixture of NO, Bra, and H, reaches equilibrium at 302 K, Pno=133 torr and Pers 151 torr. Find PNobr (in torr). [335 torr] 5. lodine gas...
The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr(g) 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 19.9 L container at 298K contains NOBr at a pressure of 0.297 atm and NO at a pressure of 0.251 atm, the equilibrium partial pressure of Br2 is ? atm.
Consider the following reaction between phosphorus trichloride and chlorine gases to make phosphorus pentachloride gas: PCl3(g) + Cl2(g) --> PCl5(g) Kp = 24.2 at 250 Celsius If the initial partial pressures of PCl3 and Cl2 are 0.43 and o.87 atm, respectively, and no PCl5 is initially present, what is partial pressure of the Cl2 when equilibrium is achieved? Simplifying assumptions cannot be made; quadratic solution is required. A. 0.00 atm B. 2.30 atm C. 0.47 atm D. 0.03 atm E....
1. (18 points) Consider the balanced gas phase combustion of dinitrotoluene, DNT (C7 HG(NO2)2): 2C7H6(NO2)2(g) + 3 O2(g) ---> 14 CO(g) +4 NH3(g). The products are carbon monoxide (CO) and ammonia (NH3). A gaseous mixture of DNT and O2(g) at 80°C is placed into a previously empty rigid container. When the above reaction goes to completion at 80°C, 0.15 atm of O2(g) is still present. The partial pressure of the NH3(g) produced is 1.00 atm. Assume all gases behave ideally....
Consider the reaction: 2 HI (g) ⇌ H₂ (g) + I₂ (g) At equilibrium, the partial pressure of HI is 1.9 atm and the partial pressures of H₂ and I₂ are 7.9 and 2.3 respectively. What is Kp for this equilibrium?
Consider the following reaction at 300 K: 2 AB (g) ↔ A2 (g) + B2 (g) In a particular experiment, the partial pressures of A2 and I2 at equilibrium are 0.715 and 0.573 atm, respectively, while the partial pressure of AB is 3.63 atm. What is the equilibrium constant for this reaction?