Highly toxic disulfur decafluoride decomposes by a freeradical process: S₂F₁₀(g) ⇒ SF₄(g) + SF₆(g). In a study of the decomposition, S₂F₁₀ was placed in a 2.0-L flask and heated to 100°C; [S₂F₁₀] was 0.50 M at equilibrium. More S₂F₁₀ was added, and when equilibrium was reattained, [S₂F₁₀] was 2.5 M. How did [SF₄] and [SF₆] change from the original to the new equilibrium position after the addition of more S₂F₁₀?

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23-08-2022
Chemistry

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Highly toxic disulfur decafluoride decomposes by a freeradical process: S₂F₁₀(g) ⇒ SF₄(g) + SF₆(g). In a study of the decomposition, S₂F₁₀ was placed in a 2.0-L flask and heated to 100°C; [S₂F₁₀] was 0.50 M at equilibrium. More S₂F₁₀ was added, and when equilibrium was reattained, [S₂F₁₀] was 2.5 M. How did [SF₄] and [SF₆] change from the original to the new equilibrium position after the addition of more S₂F₁₀?

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Tutorconsortium363 Tutorconsortium363 · Answer 1 · 2022-08-29T19:15:01+02:00

Since the Avogadro's constant gives the relation between the number of constituent particles and the amount of substance, its SI unit is the reciprocal of mole and has the value NA=6.022×1022mol−1NA=6.022×1022mol−1.

Avogadro's constant

When the Avogadro's constant's numerical value is expressed without its dimensions it gives the exact number of particles present in one mole of any substance. This is called the Avogadro's number and it has a value of N=6.022×1023N=6.022×1023.

Now, to find out the moles of disulfur decay fluoride present in 1.55×10221.55×1022 molecules, we simply have to divide this number with Avogadro's constant.

Number of moles = 1.55×10226.022×1023mol−1Number of moles ≅ 0.026 mol number of moles = 1.55×10226.022×1023mol−1Number of moles ≅ 0.026 mol

So, there are 0.026 moles present in 1.55×10221.55×1022 molecules of disulfur decay fluoride.

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