The reaction C4H8(g)⟶2C2H4(g)C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol.262 kJ/mol. At 600.0 K,600.0 K, the...

The reaction

C4H8(g)⟶2C2H4(g)C4H8(g)⟶2C2H4(g)

has an activation energy of 262 kJ/mol.262 kJ/mol. At 600.0 K,600.0 K, the rate constant, ?,k, is 6.1×10−8 s−1.6.1×10−8 s−1. What is the value of the rate constant at 765.0 K?

Solutions

Expert Solution

Value of rate constant at 765.0 K is 5.073 × 10^(-3) s^-1

Explanation :

Rate of reaction increases rapidly with increase in temperature which increases the value of rate constant .

Relationship between rate constants and temperature is given by Arrhenius equation which is used here to solve the problem .

queen_honey_blossom answered 1 year ago

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