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Korolek [52]
3 years ago
10

Which represents the correct equilibrium constant expression for the reaction below? Cu(s)+2Ag+(aq)<->Cu2+(aq)+2Ag(s)

Chemistry
2 answers:
balu736 [363]3 years ago
4 0
K(eq) = concentration of products/concentration of reactant         = [Cu+2] / [Ag+]^2 
Activity of pure solid and liquid is taken as 1.
Hence last option is correct.
Hope this helps, have a great day ahead!
I hope this helps you alot
:)
:)
:0

Schach [20]3 years ago
4 0

Answer : The correct option is, k_{eq}=\frac{[Cu^{2+}]}{[Ag^+]^2}

Explanation :

The given balanced chemical reaction is,

Cu(s)+2Ag^+(aq)\rightleftharpoons Cu^{2+}(aq)+2Ag(s)

The equilibrium expression for the reaction is determined by multiplying the concentrations of products and divided by the concentrations of the reactants and each concentration is raised to the power that is equal to the coefficient in the balanced reaction.

So, the equilibrium constant expression will be,

k_{eq}=\frac{[Cu^{2+}]}{[Ag^+]^2}

As we know that the concentrations of pure solids are constant that is they do not change. Thus, they are not included in the equilibrium expression.

Hence, the correct expression for the equilibrium constant is, k_{eq}=\frac{[Cu^{2+}]}{[Ag^+]^2}

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A solution of HNO3HNO3 is standardized by reaction with pure sodium carbonate. 2H++Na2CO3⟶2Na++H2O+CO2 2H++Na2CO3⟶2Na++H2O+CO2 A
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Answer:

(0,653±0,002) M of HNO₃

Explanation:

The reaction of standarization of HNO₃ with Na₂CO₃ is:

2 HNO₃ + Na₂CO₃ ⇒ 2 Na⁺ + H₂O + CO₂ + 2NO₃⁻

To obtain molarity of HNO₃ we need to know both moles and volume of this acid. The volume is (27,71±0,05) mL and to calculate the moles it is necessary to obtain the Na₂CO₃ moles and then convert these to HNO₃ moles, thus:

0,9585 g of Na₂CO₃ × ( 1 mole / 105,988 g) =

9,043×10⁻³ mol Na₂CO₃ × ( 2 moles of HNO₃ / 1 mole of Na₂CO₃) = 1,809×10⁻² moles of HNO₃

Molarity is moles divide liters, thus, molarity of HNO₃ is:

1,809×10⁻² moles / 0,02771 L = 0,6527 M of HNO₃

The absolute uncertainty of multiplication is the sum of relative uncertainty, thus:

ΔM = 0,6527M× (0,0007/0,9585 + 0,001/105,988 + 0,05/27,71) =

0,6527 M× 2,54×10⁻³ = 1,7×10⁻³ M

Thus, molarity of HNO₃ solution and its absolute uncertainty is:

(0,653±0,002) M of HNO₃

I hope it helps!

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