Question

For the reaction in a sealed container at a constant temperature, 2NO(g) + Br_{2}(g) ? 2NOBr(g) the initial concentrations are 4.85 M NO, 5.15 M Br_{2}, and no NOBr. At equilibrium, [NOBr] = 2.95 M. Calculate the value of K under the reaction conditions. K =

          For the reaction in a sealed container at a constant temperature,

2NO(g) + Br_{2}(g) ? 2NOBr(g)

the initial concentrations are 4.85 M NO, 5.15 M Br_{2}, and no NOBr. At equilibrium, [NOBr] = 2.95 M.

Calculate the value of K under the reaction conditions.
K =

For the reaction in a sealed container at a constant temperature,

2NO(g) + Br2(g) ? 2NOBr(g)

the initial concentrations are 4.85 M NO, 5.15 M Br2, and no NOBr. At equilibrium, [NOBr] = 2.95 M.

Calculate the value of K under the reaction conditions.
K =

Added by Brian R.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Supreeta N

09/16/2023

Step 1

Write the balanced chemical equation: 2NO(g) + Br2(g) ⇌ 2NOBr(g) Show more…

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For the reaction in a sealed container at a constant temperature: 2NO(g) + Br2(g) -> 2NOBr(g) The initial concentrations are 4.85 M NO, 5.15 M Br2, and no NOBr. At equilibrium, [NOBr] = 2.95 M. Calculate the value of K under the reaction conditions.