rachel2005smith

28.09.2021 • 

Chemistry

Which statement correctly explains why H2S is a stronger acid than water? Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, weaker base than H2O.
Sulfur (S) has a larger atomic size than oxygen (O), so H, 2, S, , is a more stable, weaker base than H, 2, O.

Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, stronger acid than H2O.
Sulfur (S) has a larger atomic size than oxygen (O), so H, 2, S, , is a more stable, stronger acid than H, 2, O.

Sulfur (S) has a larger atomic size than oxygen (O), so HS– is a more stable, stronger acid than OH–.
Sulfur (S) has a larger atomic size than oxygen (O), so HS, – , is a more stable, stronger acid than OH, –, .

Sulfur (S) has a larger atomic size than oxygen (O), so HS– is a more stable, weaker base than OH–.
Sulfur (S) has a larger atomic size than oxygen (O), so HS, – , is a more stable, weaker base than OH, –, .

Ответ:

ddrain6285

02.04.2021

Chemistry

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Enthalpy of formation of strontium chloride, SrCl = -558.1 kJ/mol

Explanation:

Sr(s) > Sr(g)       ΔHsublimation = +164 kJ/mol

Sr⁺(g) > Sr⁺(g)    First Ionization energy, IE₁ = +549 kJ/mol

Sr⁺(g) > Sr²⁺(g)    Second ionization energy, IE₂ = +1064 kJ/mol

I₂(s) > I₂(g)   ΔHsublimation = +62.4 kJ/mol

I₂(g) > 2I(g)   Bond dissociation energy, BE = +152.55 kJ/mol

2I(g) > 2I⁻(g)   Electron affinity, EA = 2 (-295.15 kJ/mol) = -590.3 kJ/mol

Sr²⁺(g) + 2I⁻(g) > SrI₂(s)    Lattice energy, LE = -1959.75 kJ/mol

Overall equation for the formation of SrCl₂ is given as:

Sr(s) + I₂(s) > SrI₂(s)    ΔHformation = ?

Enthalpy of formation, ΔHformation = (ΔHsublimation of Sr(s) + IE₁ + IE₂ + ΔHsublimation of I₂(s) + BE + EA + LE)

ΔHformation = {164 + 549 + 1064 + 62.4 + 152.55 + (-590.3) + (-1959.75)} kJ/mol

Sr(s) + I₂(s) > SrI₂(s)    ΔHformation = -558 kJ/mol

Therefore, enthalpy of formation of strontium chloride, SrCl = -558.1 kJ/mol

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