If a solution initially contains 0.260 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25 ∘C? Express your answer in
1 answer:
Answer:
2.16 × 10⁻³
Explanation:
Step 1: Given data
Concentration of the acid (Ca): 0.260 M
Acid dissociation constant (Ka): 1.80 × 10⁻⁵
Step 2: Write the acid dissociation equation
HC₂H₃O₂(aq) + H₂O(l) ⇄ C₂H₃O₂⁻(aq) + H₃O⁺(aq)
Step 3: Calculate the concentration of H₃O⁺ at equilibrium
We will use the following expression.
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Answer:
the activation energy Ea = 179.176 kJ/mol
it will take 7.0245 mins for the same food to cook in an open pot of boiling water at an altitude of 10000 feet.
Explanation:
From the given information
Thus;
Because at 113.0°C; the rate is 7 time higher than at 100°C
Hence:
1.9459 =
Ea = 179.176 kJ/mol
Thus; the activation energy Ea = 179.176 kJ/mol
b)
here;
where ;
Now;
t = 7.0245 mins
Therefore; it will take 7.0245 mins for the same food to cook in an open pot of boiling water at an altitude of 10000 feet.