The rate constant for a certain reaction is measured at two different temperatures: temperature Assuming the rate constant obeys
the Arrhenius equation, calculate the activation energy for this reaction. Round your answer to significant digits.
1 answer:
Answer:
The question has some details missing which I have shown in the attached file.
Explanation:
The concept of arrehenius equation is used to calculate the activation energy.
- Given T1 = 141.0 degree celsius = 414K and K1 = 3.3 x 10^8
- T2 = 77 degree celsius = 350K and k2 = 1.1 x 10^8
- R = 8.314
- from Arrehenius equation;
- ln(k2/k1) = -Ea/R [1/T2 - 1/T1]
- Plugging the values ;
- ln(1.1/3.3) = -Ea/8.314 [ 1/350 - 1/414]
- Ea = 20.679KJ/mol = activation energy for this reaction
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Answer: 0.100 m
Explanation:
Elevation in boiling point is given by:
= Elevation in boiling point
i= vant hoff factor
= boiling point constant
m= molality
1. For 0.100 m
, i= 3 as it is a electrolyte and dissociate to give 3 ions. and concentration of ions will be
2. For 0.100 m
, i= 2 as it is a electrolyte and dissociate to give 2 ions, concentration of ions will be
3. For 0.200 m
, i= 1 as it is a non electrolyte and does not dissociate, concentration of ions will be
4. For 0.060 m
, i= 4 as it is a electrolyte and dissociate to give 4 ions. and concentration of ions will be
Thus as concentration of solute is highest for , the elevation in boiling point is highest and thus has the highest boiling point.