The rate constant for a reaction is 0.447 L/mol s at 315k and 405.8 L/mols s at

Question

The rate constant for a reaction is 0.447 L/mol s at 315k and 405.8 L/mols s at 385 K. Using the Arrhenius equation, what is the activation energy for this reaction?

Ea= -R lnk2-lnk1/ (1/t2)-(1/t1)

Question 1 options:

1.18×104 J/mol

9.81×104 J/mol

7.03×105 J/mol

5.84×106 J/mol

Two nitric oxide molecules react with one another in an elementary reaction. What is the molecularity of this reaction?

Question 2 options:

1

2

3

4

The rate constant for a reaction is 0.447 L/mol s at 315k and 405.8 L/mols s at 385 K. Using the Arrhenius equation, what is the activation energy for this reaction?

Ea= -R lnk2-lnk1/ (1/t2)-(1/t1)

Question 1 options:

1.18×104 J/mol

9.81×104 J/mol

7.03×105 J/mol

5.84×106 J/mol

Two nitric oxide molecules react with one another in an elementary reaction. What is the molecularity of this reaction?

Question 2 options:

1

2

3

4

Explanation / Answer

Ans 1

From the Arrhenius equation

ln k2/k1 = -Ea/R (1/t2 - 1/t1)

Ea= -(R lnk2/k1)/ (1/t2)-(1/t1)

= - (8.314 J/mol·K x ln 405.8/0.447)/(1/385-1/315)K

= - 8.314 x 6.811 / (-0.000577)

= 98105.678 J/mol

= 9.81 x 10^4 J/mol

Option B is the correct answer

Ans 2

Molecularity of reaction = 2

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