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.

How could I find this using the given information ?

At a certain temperature, a 28.0-L container holds four gases in equilibrium. Their masses are 3.5 g SO3, 4.6 g SO₂, 24.5 g N₂, and 0.98 g N₂O. What is the value of the equilibrium constant at this temperature for the reaction of SO₂ with N₂O to form SO3 and N₂? Make sure you balance the reaction using the lowest whole-number coefficients. Kc = x10 TOOLS

If Kc = 0.00610 for the reaction below at 298.0 K, then what is the value of Kp? (R = 0.08314 L･bar/mol･K.) 3 A (g) + B (g) ⇌ C (g) + D (g)

6B.4(b) The equilibrium constant for the reaction N2(g) + O2(g)=2 NO(g) is 1.69×10-3 at 2300 K. A mixture consisting of 5.0 g of nitrogen and 2.0 g of oxygen in a container of volume 1.0 dm³ is heated to 2300 K and allowed to come to equilibrium. Calculate the mole fraction of NO at equilibrium.20

Please don't provide hand written solution.....

For the following reaction: A(g) + B(g) = 2 C(a) Calculate the magnitude of K, (don't report the units) assuming the following composition at equilibrium: PA = 0.438 bar PB = 0.716 bar Pc = 0.122 bar

For the reaction 2A(g) <===> B(g)+2C(g), a reaction vessel initially contains only A at a pressure of PA=895torr . At equilibrium, PA=65torr. First convert torr to atm by dividing by 760, and next use an ICE table to help calculate the value of Kp. (Assume no changes in volume or temperature.) Express your answer using two significant figures.

At 1100 K, K₂ = 0.30 for the reaction 2SO₂ (g) + O2(g) — 2SO3 (9) What is the value of K at this temperature? K=

Consider the reaction: SO, Cl2 (g) = SO2(g) + Cl2 (g) K=2.97 × 10³ at 625 K In a reaction mixture at equilibrium, the partial pressure of SO2 is 139 mbar and that of Cl2 is 286 mbar . Part A What is the partial pressure of SO2 Cl2 ? Pso,Cl2 = bar