2) For the equilibrium: 2 SO3(g) <=> O2(g) + 2 SO2(g) Kp = 0.269 at 625...

Question

Question

2) For the equilibrium: 2 SO3(g) <=> O2(g) + 2 SO2(g) Kp = 0.269 at 625 °C What is Ke at this temperature? Kp = Kc[RT]An R =

science chemistry

Answer 1

Answer #1

Kp=Kc[RT] $\Delta$ n

Kc=Kp/[RT] $\Delta$ n

$\Delta$ n= moles of gaseous product - moles of gaseous reactant = 3-2=1

625oc=898K

ie: Kc= 0.269/(0.08206 x 898)1

Kc=0.00365

Add a comment

Answer 2

Similar Homework Help Questions

2) For the equilibrium: 2 SO3(g) <=> 02(g) + 2 SO2(g) Kp = 0.269 at 625...

2) For the equilibrium: 2 SO3(g) <=> 02(g) + 2 SO2(g) Kp = 0.269 at 625 °C What is Ke at this temperature? Kp = K[R R = 0.08206 L-atm/mol K (5pts)
For the equilibrium: 2 SO3(g) < = > O2(g) + 2 SO2(g) Kp = 0.269 at...

For the equilibrium: 2 SO3(g) < = > O2(g) + 2 SO2(g) Kp = 0.269 at 625 oC What is Kc at this temperature? Kp = Kc[RT]Δn R = 0.08206 L-atm/mol K
2) For the equilibrium: 2 SO2(g) + O2(g) < => 2 503(g) Kp = 2.98 at...

2) For the equilibrium: 2 SO2(g) + O2(g) < => 2 503(g) Kp = 2.98 at 875oC What is Ke at this temperature? Ko-K[RT]An R = 0.08206 L-atm/mol K (5pts)

5. For the reaction... SO2 + O2 <=> SO3 If the equilibrium position shifts to the...

5. For the reaction... SO2 + O2 <=> SO3 If the equilibrium position shifts to the right, the concentration of O2 will (2 points) o remain constant increase Decrease
how to solve this? Sulphur trioxide decomposes at high temperature in a sealed container: 2 SO3(g)...

how to solve this? Sulphur trioxide decomposes at high temperature in a sealed container: 2 SO3(g) <--> 2 SO2(g) + O2(g). Initially, the vessel is charged at 1000 K with SO3(g) at a partial pressure of 0.500 atm. At equilibrium the SO3 partial pressure is 0.200 atm. Calculate the value of Kp at 1000 K to 3 decimal places.
For the reaction 2 SO3 (g) equilibrium reaction arrow 2 SO2 (g) + O2 (g) Kp...

For the reaction 2 SO3 (g) equilibrium reaction arrow 2 SO2 (g) + O2 (g) Kp = 0.335 at 1000 K. Calculate Kc at 1000 K. Please help.

For the equilibrium 2 SO3(g) <----> 2 SO2(g) + O2(g), Kc is 4.08 * 10-3 at...

For the equilibrium 2 SO3(g) <----> 2 SO2(g) + O2(g), Kc is 4.08 * 10-3 at 1000 K. Calculate the value for Kp.
1. 2 SO3(g) ⇄ 2 SO2(g) + O2(g) Kp = 1.2× 10-5 0.60 atm of SO3...

1. 2 SO3(g) ⇄ 2 SO2(g) + O2(g) Kp = 1.2× 10-5 0.60 atm of SO3 and 0.30 atm of SO2are placed in a container and the system is allowed to reach equilibrium. Calculate the pressure of O2(g) at equilibrium.? 2. Find the pH of 0.68 M HCOOH(aq) given that its Ka = 1.8×10-4. 2 questions please answer both
Calculate Kc for the following reaction, 2 SO2(g) + O2(g) <=> 2 SO3(g); Kp = 59.4...

Calculate Kc for the following reaction, 2 SO2(g) + O2(g) <=> 2 SO3(g); Kp = 59.4 at 12 o C Give your answer to the nearest whole number.

The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to...

The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to form SO3 is 0.365 at 1.15×103 K: SO2(g) + O2(g) = 2SO3(g) A sample of SO3 is introduced into an evacuated container at 298 K and allowed to dissociate until its partial pressure reaches an equilibrium value of 0.867 atm. Calculate the equilibrium partial pressures of SO2 and O2 in the container. PSO2 = PO2 =