Calculate kc for the reaction `2SO_2+O_2(g) ⇌ 2SO_3(g)` . kp=3.4 bar at `1000°C`, R=0.083

(i)Determine K_c for the reaction : 2SO_2(g)+O_2(g) hArr 2SO_3(g) K_p =3.4 "bar"^(-1) at 1000^@ C (ii)Determine K_p for the reaction : 2NOCl(g) hArr 2NO(g) + Cl_2(g) " " K_c=3.75xx10^(-6) at 1069 K

The equilibrium constant for the reaction: 2SO_2(g) +O_2(g) hArr 2SO_3(g) is 256 at 1000 K. What is the value of K for the reaction: SO_3(g)hArr SO_2(g) + 1/2O_2(g) at the same temperature.

The standard Gibbs energy change for the reaction 2SO_2(g) +O_2(g) to 2SO_3 (g) is -142 kJ mol^(-1) at 300 K. Calculate equilibrium constant.

The equilibrium constant, K_(p) for the reaction 2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g) is 44.0atm^(-1) "at" 1000 K . What would be the partial pressure of O_(2) if at equilibrium the amound of SO_(2) and SO_(3) is the same?

Write the relationship between K_p and K_c for the reaction 2SO_2(g) +O_2(g) hArr 2SO_3(g)

The value of K_p for the reaction, 2SO_2(g)+O_2(g) hArr 2SO_3(g) is 5 what will be the partial pressure of O_2 at equilibrium when equal moles of SO_2 and SO_3 are present at equilibrium ?

The reaction SO_(2)(g) +1//2O_(2)(g) rarr SO_(3)(g) should be