K_c = 6.5 x 10² at a particular temperature for a reaction: 2 NO(g) + 2 H(g) ⇌ N₂(g) + 2 H₂O(g). Calculate K_c at same temperature for the following reaction: 1/3 N₂(g) + 2/3 H₂O(g) ⇌ 2/3 NO(g) + 2/3 H(g).

The reaction 2 AsH31g2 ∆ As21g2 + 3 H21g2 has Kp =

7.2 * 107 at 1073 K. At the same temperature, what is Kp

for each of the following reactions?

(c) 9 H21g2 + 3 As21g2 ∆ 6 AsH31g2

The reaction 2 AsH31g2 ∆ As21g2 + 3 H21g2 has Kp =

7.2 * 107 at 1073 K. At the same temperature, what is Kp

for each of the following reactions?

(b) 4 AsH31g2 ∆ 2 As21g2 + 6 H21g2

The reaction

2 PH31g2 + As21g2 ∆ 2 AsH31g2 + P21g2

has Kp = 2.9 * 10-5 at 873 K. At the same temperature,

what is Kp for each of the following reactions?

(a) 2 AsH31g2 + P21g2 ∆ 2 PH31g2 + As21g2

Consider the following equilibrium, for which K_p = 0.0752 at 480°C: 2 Cl₂(g) + 2 H₂O(g) ⇌ 4 HCl(g) + O₂(g) (b) What is the value of K_p for the reaction Cl₂(g) + H₂O(g) ⇌ 2 HCl(g) + 1/2 O2(g)?

If K_c = 7.5×10⁻⁹ at 1000 K for the reaction N₂(g) + O₂(g) → 2 NO(g), give the value of K_c at 1000 K for the reaction

(a) 2 NO(g) → N₂(g) + O₂(g)

If K_c = 7.5×10⁻⁹ at 1000 K for the reaction N₂(g) + O₂(g) → 2 NO(g), give the value of K_c at 1000 K for the reaction

(b) NO(g) → 1/2 N₂(g) + 1/2 O₂(g)

The reaction 2 AsH31g2 ∆ As21g2 + 3 H21g2 has Kp =

7.2 * 107 at 1073 K. At the same temperature, what is Kp

for each of the following reactions?

(c) 9 H21g2 + 3 As21g2 ∆ 6 AsH31g2