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Vedmedyk [2.9K]
3 years ago
8

Consider this equilibrium: COCl2(g) CO(g) + Cl2(g) Keq = 8.1 x 10-4. What is true for this system?

Chemistry
1 answer:
fiasKO [112]3 years ago
6 0
Answer is: [COCl₂] > [CO][Cl₂]
Chemical reaction: COCl₂(g) ⇄ CO(g) + Cl₂(g); Keq = 8.1 x 10⁻⁴.
Keq = [CO] · [Cl₂] / [COCl₂]; equilibrrium constant of chemical reaction.
[CO] · [Cl₂] / [COCl₂] = 0,00081.
Equilibrium product concentration is much more less than equilibrium concentration of reactant.

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A mixture of three noble gases has a total pressure of 1.25 atm. The individual pressures exerted by neon and argon are 0.68
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First of all, as you seen the gases are noble which means that will not react with each other and in this case each gas create individual pressure.  

P_{T}= total pressure  

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P_{T} = P_{Ne} + P_{Ar} + P_{He}    

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Given the following balanced equation, if the rate of O2 loss is 3.64 × 10-3 M/s, what is the rate of formation of SO3? 2 SO2(g)
Fynjy0 [20]

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Rate of formation of SO₃ [\frac{d[SO_{3}] }{dt}] = 7.28 x 10⁻³ M/s

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According to equation   2 SO₂(g) + O₂(g) → 2 SO₃(g)

Rate of disappearance of reactants = rate of appearance of products

                     ⇒ -\frac{1}{2} \frac{d[SO_{2} ]}{dt} = -\frac{d[O_{2} ]}{dt}=\frac{1}{2} \frac{d[SO_{3} ]}{dt}  -----------------------------(1)

    Given that the rate of disappearance of oxygen = -\frac{d[O_{2} ]}{dt} = 3.64 x 10⁻³ M/s

             So the rate of formation of SO₃ [\frac{d[SO_{3}] }{dt}] = ?

from equation (1) we can write

                                   \frac{d[SO_{3}] }{dt} = 2 [-\frac{d[O_{2}] }{dt} ]

                                ⇒ \frac{d[SO_{3}] }{dt} = 2 x 3.64 x 10⁻³ M/s

                                ⇒ [\frac{d[SO_{3}] }{dt}] = 7.28 x 10⁻³ M/s

∴ So the rate of formation of SO₃ [\frac{d[SO_{3}] }{dt}] = 7.28 x 10⁻³ M/s

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