A certain reaction has an activation energy of 67.0 kJ/mol and a frequency factor of A1 = 4.20×1012. What is the rate constant,
1 answer:
Answer:
- K = 7.00
Explanation:
<u>1) Arrhenius equation</u>
Arrhenius equation shows the relation between activation energy, temperature, and the equilibrium constant.
This is the equation:
Where:
- K is the equilibrium constant,
- A is the frequency factor,
- Ea is the activation energy (in J/mol),
- T is the temperature in kelvins (K), and
- R is the universal constant.
<u></u>
<u>2) Substitute, using the right units, and compute:</u>
- A = 4.20 × 10¹² (dimensionless)
- Ea = 67.0 kJ/mol = 67,000 J/mol
- T = 24.0°C = 24.0 + 273.15 K = 297.15 K
- R = 8.314 J/K mol
- K = 7.00
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When sodium phosphate reacts with sulfuric acid, forming sodium sulfate and phosphoric acid, the stoichiometric coefficient for sulfuric acid in the balanced chemical equation is 3.
In every balanced chemical equation, the total number of individual atoms on the reactant side must be equal to the total number of individual atoms on the product side. The stoichiometric coefficient is the number written in front of each reactants and products that tells how many moles of each are needed in the reaction.
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Put the necessary stoichiometric coefficient to balance each element.
Balancing Na:
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=
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where 3 is the stoichiometric coefficient of sulfuric acid, .
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