The reaction h2co3 h2o<-> h3o hco3– takes place in water. what happens to the equilibrium when the pressure is increased?
2 answers:
Answer: It does not change.
Explanation:
According to Le Chatelier's principle, if an equilibrium reaction is subjected to a change, the reaction adjusts itself in a way to undo the change imposed.
The effect of pressure affects the equilibrium only when the reactants or products are in gaseous phase.
As none of the reactants or products is in gaseous state, there is no effect of pressure on equilibrium.
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Answer:
Molar absorptivity or molar extinction co-effecient = 2120.14 cm⁻¹M⁻¹
Explanation:
First convert Concentration from ppm inM or mol/l
⇒ Molar mass of KMnO₄ = 158.03 g
⇒ 4.48 ppm = 4.48 mg/l = 4.48 x 10⁻³ g/l
⇒ Molarity = = 2.83 x 10⁻⁵ molar
Absorbance (A) = - log(T) ( T = % transmittance)
= - log(0.859)
= 0.06
According to Lambert Beer's law
ε =
or, ε =
or, ε = 2120.14 cm⁻¹M⁻¹
Where
ε = Molar absorptivity
A = absorbance
C = Molar concentration of KMnO₄ solution
l = length