Answer:
118.4 g
Explanation:
4 Ga + 3 S₂ → 2 Ga₂S₃
According to the equation, for every 4 moles of gallium burned, 2 moles of gallium(III) sulfide.
First, convert grams of Ga₂S₃ to moles. The molar mass is 235.641 g/mol.
(200.0 g)/(235.641 g/mol) = 0.8487 mol
Use the relationship above to convert moles of Ga₂S₃ to moles of Ga.
(0.8487 mol Ga₂S₃) × (4 mol Ga)/(2 mol Ga₂S₃) = 1.697 mol Ga
Convert moles of Ga to grams. The molar mass is 69.723 g/mol.
(1.697 mol Ga) × (69.723 g/mol) = 118.4 g
The answer is caso4 and ca(C2H3O2)2
Given data:
Sublimation of K
K(s) ↔ K(g) ΔH(sub) = 89.0 kj/mol
Ionization energy for K
K(s) → K⁺ + e⁻ IE(K) = 419 Kj/mol
Electron affinity for Cl
Cl(g) + e⁻ → Cl⁻ EA(Cl) = -349 kj/mol
Bond energy for Cl₂
1/2Cl₂ (g) → Cl Bond energy = 243/2 = 121.5 kj/mol
Formation of KCl
K(s) + 1/2Cl₂(g) → KCl(s) ΔHf = -436.5 kJ/mol
<u>To determine:</u>
Lattice energy of KCl
K⁺(g) + Cl⁻(g) → KCl (s) U(KCl) = ?
<u>Explanation:</u>
The enthalpy of formation of KCl can be expressed in terms of the sum of all the above processes, i.e.
ΔHf(KCl) = U(KCl) + ΔH(sub) + IE(K) + 1/2 BE(Cl₂) + EA(Cl)
therefore:
U(KCl) = ΔHf(KCl) - [ΔH(sub) + IE(K) + 1/2 BE(Cl₂) + EA(Cl)]
= -436.5 - [89 + 419 + 243/2 -349] = -717 kJ/mol
Ans: the lattice energy of KCl = -717 kj/mol
The required volume of 0.10M NaOH solution that student will add is 20 mL.
<h3>How do we calculate the volume?</h3>
Volume of any solution which is required to prepare buffer will be calculated by using the below equation as:
M₁V₁ = M₂V₂, where
- M₁ & V₁ are the molarity and volume of NaOH solution.
- M₂ & V₂ are the molarity and volume of HF solution.
On putting values, we get
V₁ = (0.1)(20) / (0.1) = 20mL
Hence required volume of NaOH solution is 20mL.
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