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mars1129 [50]
3 years ago
10

FILL IN THE BLANKWORD BANK (can use more than once): less, increases, decreases, greaterNO2Cl(g)+NO(g)⇌NOCl(g)+NO2(g)1.Disturbin

g the equilibrium by adding NO2Cl ____ Qc to a value ____ than Kc.2.To reach a new state of equilibrium, Qc therefore ____ , which means that the denominator of the expression for Qc _____.3.To accomplish this, the concentration of reagents ____ , and the concentration of products ____.
Chemistry
1 answer:
Jlenok [28]3 years ago
4 0

Explanation:

If we have the following reaction at equilibrium:

<em>                                           aA + bB ⇄ cC + dD</em>

where a, b, c, and d are the stoichiometric coefficients for the reacting species A, B,  C, and D. For the reaction at a particular temperature:

                       Kc=([C]^c *[D]^d)/([A]^a *[B]^b)

where Kc is the equilibrium constant, which holds that <em>for a reversible reaction at equilibrium  and a constant temperature, a certain ratio of reactant and product concentrations has  a constant value, Kc</em> (the equilibrium constant). Note that although the concentrations  may vary, as long as the reaction in in equilibrium and temperatura don't change, the value of <u>K remains constant.</u>

For reactions that have not reached equilibrium, we obtain the reaction quotient (Qc), instead of the equilibrium  constant <u>by substituting the initial concentrations into the equilibrium constant expression.</u>

                        Qc=([Co]^c *[Do]^d)/([Ao]^a *[Bo]^b)

To determine the direction in wich the net reaction will proceed to reach equilibrium, que compare the values of Qc and Kc.

  • Qc < Kc: To reach equilibrium, reactants must be converted to products (→)
  • Qc = Kc: The initial concentrations are equilibrium concentrations. The system in at equilibrium.
  • Qc > Kc: To reach equilibrium, products must be converted to reactants (←)

Solution:

We have the following reaction:

                             NO2Cl(g)+NO(g)⇌NOCl(g)+NO2(g)

So:

Kc=([NOCl]^1*[NO2]^1)/([NO2Cl]^1 *[NO]^1)

     =([NOCl][NO2])/([NO2Cl][NO])  

1. In the equation above, [NO2Cl] it's in the denominator, so if we increase it's numericall value by adding NO2Cl <u>decreases Qc  to a value less than Kc.</u>

<em>(From the chemical point of view, if we disturb the equilibrium adding NO2Cl (a reactant), to reach equilibrium again the system proceeds from left to right (→) consuming this reactant.)</em>

2. To reach a new state of equilibrium (<em>where Qc = Kc</em>), Qc therefore  increases wich means that the denominator of the expression for Qc  decreases <em>(in order to increase the denominator as mention above).</em>

3. To accomplish this, the concentration of reageants decreases <em>(reagents are being consumed), </em>and the concentration of prodcuts increases <em>(products are being formed).</em>

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