Answer:
of the reaction is -6313 kJ/mol
of the reaction is -6312 kJ/mol
Explanation:





Therefore,
of the reaction is -6313 kJ/mol.
The chemical reaction in bomb calorimeter is as follows.




Therefore,
of the reaction is -6312 kJ/mol.
Answer:
The final molarity of acetate anion in the solution is 0.0046 moles
Explanation:
The balanced equation is
Cu(C₂H₃O₂)₂ + Na₂CrO₄ = CuCrO₄ + 2Na(C₂H₃O₂)
Therefore one mole of Cu(C₂H₃O₂)₂ react with one mole of Na₂CrO₄ to form one mole of CuCrO₄ and two moles of Na(C₂H₃O₂)
Mass of copper (II) acetate present = 0.708 g
Volume of aqueous sodium present = 50 mL
Molarity of sodium chromate = 46.0 mM
Therefore
Number of moles of sodium chromate present = (50 mL/1000)×46/1000 = 0.0023 M
Number of moles of copper (II) acetate present = 181.63 g/mol
number of moles of copper (II) acetate present = (0.708 g/181.63 g/mol) =0.0039 moles
Therefore 0.0039 moles of Cu(C₂H₃O₂)₂ × (2 moles of Na(C₂H₃O₂))/1 Cu(C₂H₃O₂)₂) = 0.00779 moles of Na(C₂H₃O₂)
also 0.0023 moles of Na₂CrO₄ × (2 moles of Na(C₂H₃O₂))/1 Na₂CrO₄) = 0.0046 moles of Na(C₂H₃O₂)
Therefore the Na₂CrO₄ is the limiting reactant and 0.0046 moles of Na(C₂H₃O₂) or acetate anion is formed
Answer:
3.68 g
Explanation:
= 18 ÷ 44 = 0.4
2C2H2 + 5O2 → 4CO2 + 2H2O
2 : 5 : 4 : 2
0.409 (moles)
⇒
= 0.409 × 2 ÷ 4 = 0.2045 moles
⇒
= 0.2045 × 18 = 3.68 grams
Hello!
The chemical reaction for the dissociation of Acetic Acid is the following:
CH₃COOH + H₂O ⇄ CH₃COO⁻ + H₃O⁺
To solve the problem we are going to use the Henderson-Hasselbach Equation, as follows, but first we need to know the pKa:

![pH=pKa + log( \frac{[CH_3COO^{-} ]}{[CH_3COOH]} )](https://tex.z-dn.net/?f=pH%3DpKa%20%2B%20log%28%20%5Cfrac%7B%5BCH_3COO%5E%7B-%7D%20%5D%7D%7B%5BCH_3COOH%5D%7D%20%29)

So, the pH of this solution is
5,24Have a nice day!