2.50 mol NOCI were placed in a 2.50 L reaction vessel at 400°C. After equilibrium was established, it was found that 28 percent of the NOCI had dissociated according to the equation: 2NOCI(g) — 2NO(g) + Cl₂(g) Calculate the equilibrium constant Ke for the reaction. a) 0.021 b) 0.039 c) 0.169 d) 25 e) 47 f) 0.0059 g) 0.47 h) 0.85
2.50 mol NOCI were placed in a 2.50 L reaction vessel at 400°C. After equilibrium was established, it was found that 28 percent of the NOCI had dissociated according to the equation: 2NOCI(g) — 2NO(g) + Cl₂(g) Calculate the equilibrium constant Ke for the reaction. a) 0.021 b) 0.039 c) 0.169 d) 25 e) 47 f) 0.0059 g) 0.47 h) 0.85
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Chapter1: Chemical Foundations
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![2.50 mol NOCI were placed in a 2.50 L reaction vessel at 400°C. After equilibrium
was established, it was found that 28 percent of the NOCI had dissociated according
to the equation: 2NOCI(g) — 2NO(g) + Cl₂(g)
Calculate the equilibrium constant Ke for the reaction.
a) 0.021 b) 0.039 c) 0.169 d) 25 e) 47 f) 0.0059 g) 0.47 h) 0.85](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F637a8243-98d2-45ca-8dd1-4e9d7d0f97ca%2F0c84c7c1-1eb7-4434-811d-3cc72ce22600%2Fos68tnu.jpeg&w=3840&q=75)
Transcribed Image Text:2.50 mol NOCI were placed in a 2.50 L reaction vessel at 400°C. After equilibrium
was established, it was found that 28 percent of the NOCI had dissociated according
to the equation: 2NOCI(g) — 2NO(g) + Cl₂(g)
Calculate the equilibrium constant Ke for the reaction.
a) 0.021 b) 0.039 c) 0.169 d) 25 e) 47 f) 0.0059 g) 0.47 h) 0.85
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