Answer:
The correct answer is 2.016 x 10⁻¹⁷
Explanation:
We have the following chemical reactions and their equilibrium constants (K):
(1) H₂CO₃(aq) + H₂O ⇒ H₃O⁺(aq) + HCO₃⁻(aq) K₁= 4.20×10⁻⁷
(2) HCO₃⁻(aq) + H₂O ⇒ H₃O⁺(aq) + CO₃²⁻(aq) K₂= 4.80×10⁻¹¹
And we have to obtain K for the following reaction:
H₂CO₃(aq) + 2H₂O ⇒ 2H₃O⁺(aq) + CO₃²⁻(aq)
If we add equations (1) and (2) we obtain the the desired equation. Remember that when we add chemical equations, the global equilibrium constant is the product of the constants.
H₂CO₃(aq) + H₂O ⇒ H₃O⁺(aq) + <em><u>HCO₃⁻(aq)</u></em> K₁= 4.20×10⁻⁷
+
<em><u>HCO₃⁻(aq)</u></em> + H₂O ⇒ H₃O⁺(aq) + CO₃²⁻(aq) K₂= 4.80×10⁻¹¹
-------------------------------------------------------------
H₂CO₃(aq) + 2H₂O ⇒ 2H₃O⁺(aq) + CO₃²⁻(aq) K= K₁ x K₂
K = K₁ x K₂ = (4.20×10⁻⁷) x (4.80×10⁻¹¹) = 2.016 x 10⁻¹⁷
Answer:
Explanation:
Hello!
In this case, we consider the given reaction to realize there is a 5:4 mole ratio between oxygen and nitrogen monoxide; thus, we infer that, at STP conditions, such mole ratio is eligible as a volume ratio too; therefore, the produced liters of nitrogen monoxide gas is:
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Answer:
The answer is Hide From Predators !!
Explanation:
Took the test it's correct :)
Answer:
[CO₂] = [NO] ≈ 0.11 mol/dm³
[CO] = 0.25 mol/(25 L) = 0.01 mol/dm³
[NO₂] = 0.45 mol/(25 L) = 0.018 mol/dm³
Explanation:
The number of moles of CO = 0.25 moles
The number of moles of NO₂ = 0045 moles
The temperature of the vessel = 350°C
The equilibrium constant, Kc = 67.5
We have;
The product of the the concentration of the products = Kc × The product of the concentration of the reactants, therefore;
[CO₂] × [NO] = 67.5 ×(0.25/25 × 0.45/25) = 0.01215
Given that [CO₂] = [NO], we get;
[CO₂] = [NO] = √0.01215 ≈ 0.11 mol/dm³
[CO] = 0.25 mol/(25 L) = 0.01 mol/dm³
[NO₂] = 0.45 mol/(25 L) = 0.018 mol/dm³
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