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Explanation:
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The heat absorbed when 1 mol of CS₂(g) forms from its elements at these conditions is 117.4 kJ.
Given,
Number of moles CS₂ = 1 mol
Temperature = 25° = 273 +25 = 298 Kelvin
Heat absorbed = 89.7 kJ
It takes 27.7 kJ to vaporize 1 mol of the liquid
Calculate the heat absorbed:
C(s) + 2S(s) → CS₂(l) ΔH = 89.7 kJ (positive since heat is absorbed)
CS₂(l) → CS₂g) ΔH = 27.7 kJ (positive since heat is absorbed)
Prior to summing, the equations should be balanced; however, because they are balanced already, there is nothing further we need to do.
C(s) + 2S(s)---> CS₂ (g)
ΔH = 89.7 + 27.7 = 117.4 kJ
Hence, the heat absorbed is 117.4 kJ.
To know more about heat absorbed refer to: brainly.com/question/9588553
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Reaction of dissociation: Ag₂SO₄ → 2Ag⁺ + SO₄²⁻.
m(Ag₂SO₄) = 4 g.
V(Ag₂SO₄) = 1 l.
n(Ag₂SO₄) = m(Ag₂SO₄) ÷ M(Ag₂SO₄).
n(Ag₂SO₄) = 4 g ÷ 311,8 g/mol.
n(Ag₂SO₄) = 0,0128 mol.
n(Ag⁺) = 2 · 0,0128 mol = 0,0256 mol.
n(Ag₂SO₄) = n(SO₄²⁻) = 0,0128 mol.
c(Ag⁺) = n ÷ V = 0,0256 mol ÷ 1 l = 0,0256 mol/l.
Ksp = c(Ag⁺)² · c(SO₄²⁻).
Ksp = (0,0256 mol/l)² · 0,0128 mol/l.
Ksp = 8,3·10⁻⁶.
