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1) Which of the following reactions would be fastest in the forward direction?
A) Ea = 50 kJ/mol; E = 20 kJ/mol.
B) Ea = 80 kJ/mol; E = 10 kJ/mol.
C) Ea = 40 kJ/mol; E = -30 kJ/mol.
D) Ea = 60 kJ/mol; E = -80 kJ/mol.
2) Which of the following reactions would be slowest in the forward direction?
A) Ea = 50 kJ/mol; E = 20 kJ/mol.
B) Ea = 80 kJ/mol; E = 10 kJ/mol.
C) Ea = 40 kJ/mol; E = -30 kJ/mol.
D. Ea = 60 kJ/mol; E = -80 kJ/mol.
3) Which of the following reactions would be fastest in the reverse direction?
A) Ea = 50 kJ/mol; E = 20 kJ/mol.
B) Ea = 80 kJ/mol; E = 10 kJ/mol.
C) Ea = 40 kJ/mol; E = -30 kJ/mol.
D) Ea = 60 kJ/mol; E = -80 kJ/mol.
4) Which of the following reactions would be slowest in the reverse direction?
A) Ea = 50 kJ/mol; E = 20 kJ/mol.
B) Ea = 80 kJ/mol; E = 10 kJ/mol.
C) Ea = 40 kJ/mol; E = -30 kJ/mol.
D) Ea = 60 kJ/mol; E = -80 kJ/mol.

Answer :

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Answer:

1) C) Ea = 40 kJ/mol; E = -30 kJ/mol.

2) B) Ea = 80 kJ/mol; E = 10 kJ/mol.

3) Ea = 40 kJ/mol; E = -30 kJ/mol.

4) B) Ea = 80 kJ/mol; E = 10 kJ/mol.

Explanation:

The activation energy Ea is the energy that reactants must possess in order to cross the 'energy barrier' between reactants and products.

The rate of reaction depends on the activation energy as we can see from the Arrhenius equation; k = Ae^-Ea/RT. The higher the activation energy, the slower the rate of reaction.

If this is the case, then the reaction with the lowest activation energy is the fastest in any given direction while the reaction with the highest activation energy is the slowest in any given direction, hence the answers above.

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