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Butoxors [25]
3 years ago
11

For the reaction COCl2(g)⇌CO(g)+Cl2(g), K= 2.19×10−10 at 373 K

Chemistry
1 answer:
vladimir1956 [14]3 years ago
6 0

Answer:

D) The equilibrium lies far to the left

Explanation:

According to the law of mass action, the equilibrium constant K for the reaction at 373K can be calculated as follows:

K = \frac{[CO][Cl_{2}]}{[COCl_{2}]} = 2.19×10^{-10}

([X] means = concentration of X)

This means that in the equilibrium the concentration of the reactant (that is in the denominator) will be much higher (around 10^{10} fold) than the concentrations of the products (that are in the numerator), and this means that the equilibrium lies far to the left (to the reactants side) as very small amount of product is being formed.

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2.0 mol of oxygen are consumed.

Step-by-step explanation:

You know that you will need a balanced equation with masses, moles, and molar masses, so gather all the information in one place.

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<em>Step 3.</em> Calculate the amount of heat generated.

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The conversion factor is 67.6 kcal/1 mol CO₂

q = 4.00 × 67.6

q = 270 kJ

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Option D is <em>wrong. </em>

<em> </em>

<em>Step 6</em>. Calculate the moles of O₂ produced

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Moles of O₂ = 2.00 mol O₂

Option E is <em>wrong. </em>

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3 years ago
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