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Aleksandr-060686 [28]
3 years ago
12

Calculate the rate constant at 200.°C for a reaction that has a rate constant of 8.30 × 10−4 s−1 at 90.°C and an activation ener

gy of 56.8 kJ/mol.
Chemistry
1 answer:
Sergeu [11.5K]3 years ago
4 0

Answer:

23.0 s⁻¹ is rate constant

Explanation:

Using the Arrhenius equation:

k = A * e^(-Ea/RT)

Where k is rate constant

A is frequency factor (1.5x10¹¹s⁻¹)

Ea is activation energy = 55800J/mol

R is gas constant (8.314J/molK)

And T is absolute temperature (24°C + 273 = 297K)

Replacing:

k = 1.5x10¹¹s⁻¹ * e^(-55800J/mol/8.314J/molK*297K)

k = 1.5x10¹¹s⁻¹ * 1.53x10⁻¹⁰

k = 23.0 s⁻¹ is rate constant    i hope this helpsss

Explanation:

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Answer:true

true

Explanation:

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If a solution containing A+ ions and a solution containing B- ions have just been mixed and [A+][B-] is greater than Ksp of AB,
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Answer:

Explanation:

In the solution of AB , they are split  to give ions as follows

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Product of concentration of A⁺ and B⁻ in saturated solution of AB is constant .

This is called Ksp

Ksp = [A⁺] [ B⁻]

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2 years ago
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Answer:

Throughout the explanation section, the reason behind the given statement is described.

Explanation:

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4 0
3 years ago
A certain metal M forms a soluble sulfate salt MSO, Suppose the left half cell of a galvanic cell apparatus is filled with a 3.0
bija089 [108]

Answer:

E = 0.062 V

Explanation:

(a) See the attached file for the answer

(b)

Calculating the voltage (E) using the formula;

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Where,

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Substituting, we have

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5 0
2 years ago
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