Answer:
6.75 × 10⁻⁸is the value of the equilibrium constant at this temperature.
Explanation:
2H₂O(g) ⇄ 2H₂(g) + O₂(g)
Partial pressure of H₂O = 0.0500 atm
Partial pressure of H₂ = 0.00150 atm
Partial pressure of O₂ = 0.00150 atm
The expression of Kp for the given chemical equation is:
![K_p = \frac{[H_2]^2[O_2]}{H_2O}](https://tex.z-dn.net/?f=K_p%20%3D%20%5Cfrac%7B%5BH_2%5D%5E2%5BO_2%5D%7D%7BH_2O%7D)
6.75 × 10⁻⁸is the value of the equilibrium constant at this temperature
The mass of 5.2 x 10^22 manganese atoms in grams would be 635.784 grams.
What is Avogadro's constant?
Avogadro's number tells us how many particles are in one mole (or mol) of a substance. <u>Electrons</u><u>, molecules, or atoms</u> could be among these particles. Avogadro's number has a value of approximately 6.022140857×10²³ mol⁻¹. Avogadro's number tells us how many particles are in one mole (or mol) of a substance. <u>Electrons, molecules, or atoms </u>could be among these particles. Avogadro's number has a value of approximately 6.022140857×10²³.
Computation of mass
Avogadro calculated that every material had 6.022 x 10^23 atoms per mole.
5.2 x 10^22 atoms of Mn would contain how many moles?
= 6.022 x 10^23 /1 x 5.2 x10^22
=11.58 moles
Mn mass equals 11.58 moles multiplied by 54.9
= 635.784 grams
You may learn more about Avogadro's constant here: brainly.com/question/15989275
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Explanation:
accuracy measurements are important because precise amount are required for reaction to take place
