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2 years ago

The rate constant for a first order reaction

Chemistry

1 answer:

Lena [83]2 years ago

8 0

Answer:

E_a = 103.626 × 10³ KJ/mol

Explanation:

Formula to solve this is given by;

Log(k2/k1) = (E_a/2.303R)((1/T1) - (1/T2))

Where;

k2 is rate constant at second temperature

k1 is rate constant at first temperature

R is universal gas constant

T1 is first temperature

T2 is second temperature

We are given;

k1 = 2.8 × 10^(-3) /s

k2 = 4.8 × 10^(-4) /s

R = 8.314 J/mol.k

T1 = 60°C = 333.15 K

T2 = 45°C = 318.15 K

Thus;

Log((4.8 × 10^(-4))/(2.8 × 10^(-3))) = (E_a/(2.303 × 8.314))((1/333.15) - (1/318.15))

We now have;

-0.76592 = -0.00000739121E_a

E_a = -0.76592/-0.00000739121

E_a = 103.626 × 10³ KJ/mol

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3 years ago

The energy E of the electron in a hydrogen atom can be calculated from the Bohr formula: E = R_y/n^2 In this equation R_y stands

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Answer:

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Explanation:

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2 years ago

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Vinil7 [7]

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