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12 Dec 2019

For the following reaction the equilibrium constant Kc-is 2.0 at a certain temp. Write the equilibrium constant expression of the equilibrium constant Kc-.
2NOBr(g) ------2NO(g)+Br2(g)

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Elin Hessel
Elin HesselLv2
13 Dec 2019

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Related questions

Nitrosyl bromide, NOBr, is formed in the reaction of nitric oxide,NO, with bromine,Br2 : 2NO(g)+Br(g)<---->2NOBr(g) Thereaction rapidly establishes equilibrium when the reactants aremixed. At a certain temperature the concentration of was 0.400M andthat of Br2 was 0.255M . At equilibrium the concentration of NOBrwas found to be 0.250M . What is the value of Kc at thistemperature?

Consider the following system at equilibrium where H° = -16.1 kJ, and Kc = 6.50×10^-3, at 298 K.

2NOBr(g) <-->2NO(g) + Br2(g)

When 0.19 moles of NOBr (g) are added to the equilibrium system at constant temperature the value of Kc:

The value of Kc:

A. increases. B. decreases. C. remains the same.

The value of Qc:

A. is greater than Kc. B. is equal to Kc. C. is less than Kc.

The reaction must:

A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium.

The number of moles of NO will:

A. increase. B. decrease. C. remain the same.

In an analysis of the following reaction at a certain temperature,

Br2(g) + Cl2(g) ⇌ 2BrCl(g)


the equilibrium concentrations were found to be [Br2] = 2.6 × 10−3 M, [Cl2] = 2.4 × 10−2M, and [BrCl] = 2.4 × 10−2 M. Write the equilibrium expression, and calculate the equilibrium constant for this reaction at this temperature.

Kc = ____/____

Kc = _____

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