Carbonyl bromide can dissociate into carbon monoxide and bromine: COBr2(g) CO(g) + Br2(g) At 73 °C, the equilibrium constant in terms of pressures, K, for this dissociation reaction is 5.40. (a) If 19.96 g of carbonyl bromide is placed in a 16.03-L vessel and heated to 73 °C, what is the partial pressure of carbon monoxide when equilibrium is attained? 0.00641 atm (b) What fraction of carbonyl bromide is dissociated at equilibrium? 0.968
Carbonyl bromide can dissociate into carbon monoxide and bromine: COBr2(g) CO(g) + Br2(g) At 73 °C, the equilibrium constant in terms of pressures, K, for this dissociation reaction is 5.40. (a) If 19.96 g of carbonyl bromide is placed in a 16.03-L vessel and heated to 73 °C, what is the partial pressure of carbon monoxide when equilibrium is attained? 0.00641 atm (b) What fraction of carbonyl bromide is dissociated at equilibrium? 0.968
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...
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Carbonyl bromide can dissociate into carbon monoxide and bromine
At 73 °C, the equilibrium constant in terms of pressures, Kp, for this dissociation reaction is 5.40.
If 19.96 g of carbonyl bromide is placed in a 16.03-L vessel and heated to 73 °C, what is the partial pressure of carbon monoxide when equilibrium is attained?
What fraction of carbonyl bromide is dissociated at equilibrium?
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