if the initial pressure of A was 1.71atm, what would the partial pressure of A(in atms) at equilibrium? Kp=58 at 298K 2A(g)B(g)+C(g)

For the equilibrium 3H₂(g)+N₂(g) P -0.00239 atm, P," NH₂ -0.763 atm and P 2NH, (g), the equilibrium partial pressures are = 0.921 atm, at 500°C. Calculate Kp.

In the reaction below, 5 atm of H2 and 1 atm of Cl2 were placed into a 1.00 L flask and allowed to react: H2(g) + Cl2(g) <=> 2 HCl(g) Given that Kp at 900 K is K = 16, calculate the equilibrium pressure of HCl and give to 2 decimal places.

Nitrogen dioxide reacts to form dinitrogen tetroxide as follows: 2 NO2 N₂04 (g) At 150 °C, Kp = 4.51. If one starts with 10.0 atm NO2 (g), what is the equilibrium pressure (in atm) of N₂O4 (g)?

A gas mixture consisting of 1.05 Atm of SO3 and 0.425 Atm of O2 was placed in a container and after the equilibrium 2SO2 (g) + O2 (g) ⇄ 2SO3 (g) was established, the total pressure was 1.62 Atm. What is the equilibrium constant, Kp?

(b) At 100° C, the Keq for the Haber process is 4,51 X 10-5: N₂ + 3 H₂ 2 NH3 Consider the following reaction conditions and determine if the system is at equilibrium. If not, indicate the direction in which the reaction must proceed to establish equilibrium (i) PNH3 105 atm, PN2 = 35 atm and PH2 = 495 atm (ii) PNH3 35 atm, PN2 = 0 atm and PH2 = 595 atm (iii) PNH3 = 26 atm, PN2 = 202 atm and PH2 = 42 atm (iv) PNH3 105 atm, PN2 = 5 atm and PH2 = 55 atm

The equilibrium constant for the following reaction is 67.6 at 232 °C. PCI3(g) + Cl₂(g)=PC15(g) K 67.6 at 232 °C Calculate the equilibrium constant for the following reactions at 232 °C. (a) PCI5(g) PCI3(g) + Cl₂(g) K= (b) 2 PCI,(g)2 PCI3(g) + 2 Cl₂(g) K=

25.00 g of solid ammonium hydrogen sulfide is introduced into a 750.-mL flask at 25°C, the flask is sealed, and the system is allowed to reach equilibrium.  What is the partial pressure of ammonia in this flask if Kp = 0.108 at 25°C for NH4HS(s) (equilibrium sign) NH3(g) + H2S (g)?

Liquid N2O3 is dark blue at low temperatures, but the color fades and becomes greenish at higher temperatures as the compound decomposes to NO and NO2. At 25 °C, a value of KP = 1.91 has been established for thisdecomposition. If 0.236 moles of N2O3 are placed in a 1.52-L vessel at 25 °C, calculate the equilibrium partial pressures of N2O3(g), NO2(g), and NO(g).