The partial pressures at equilibrium are: = 0.001915 atm Po. Pso, = 0.003132 atm Pso, = 0.0166 atm Calculate Kp for the reaction.

A reaction vessel contains an equilibrium mixture of SO2, O2, and SO3. The reaction proceeds such that:2SO2​(g)+O2​(g)<--->2SO3​(g) The partial pressures at equilibrium are:  PSO2​​=0.001111 atm   PO2​​=0.002728 atm   PSO3​​=0.0166 atm  Calculate KP for the reaction.

For the following heterogeneous equilibrium at 800 degrees C: CaCO3(s) <--> CaO(s) + CO2-(g) the pressure of CO2 is 0.236 atm.  Calculate:  (a) Kp and (b) Kc for the reaction at this temperature.  (Hint: R= 0.08206 L·atm/mol·K )

A reaction vessel contains an equilibrium mixture of SO2, O2, and SO3. The reaction proceeds such that: The partial pressures at equilibrium are:  PSO2​​=0.001714 atm   PO2​​=0.001919 atm   PSO3​​=0.0166 atm   Calculate KP for the reaction.

An empty steel container is filled with 0.880 atm of A and 0.880 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) PrtScn Home

The Haber process involves the following reaction: N2 (g) + 3H2 (g) ⇌ 2NH3 (g) N2 and H2 in the mole ratio of 1:3 were mixed in a closed container and allowed to achieve equilibrium at 450 oC. The equilibrium mixture was found to contain 15% of ammonia and the total pressure in the container is 10 atm. Calculate the equilibrium constant, Kp of the reaction.

The partial pressures at equilibrium are: = 0.001714 atm P Pso₂ Po₂ = 0.001717 atm Pso₂ = 0.0166 atm Calculate Kp for the reaction. See Periodic Table See Hint

c. In a different equilibrium mixture, under different conditions, the partial pressures of the gases are shown in the table: Gas Partial pressure / kPa N2 1.20 x 102 H2 1.50 x 102 NH3 1.10 x 103 Calculate the value of the equilibrium constant (Kp) for this reaction and give its units. d. The enthalpy change for the reaction is -92 kJ mol-1 State the effect, if any, of an increase in temperature on the value of Kp for this reaction. Explain your answer. 3. a. Name the catalyst used in the Haber process. b. Explain why a catalyst does not change the yield of ammonia produced. c. Sketch a Maxwell Boltzmann distribution curve (with labelled axes) and use it to explain why a catalyst will increase the rate of reaction.

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