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Juliette [100K]
2 years ago
11

Use the following to calculate ΔH°latice of MgF₂:

Chemistry
1 answer:
mash [69]2 years ago
7 0

Yes, Since magnesium ions have a charge that is two times greater than that of lithium and sodium ions, MgF2 has higher lattice energy than LiF and NaCl.

Lattice energy: MgF2 (s) → Mg2+(g) + 2 F–(g)

Use Hess’s law:                                      

∆Hº Mg(s) → Mg(g)                                  

Mg(s) → Mg(g) ΔH° = 148kJ F₂(g) → 2F(g) ΔH° = 159kJ

M(g) → Mg⁺ (g) + e⁻ ΔH° = 738kJ

M⁺(g) → Mg²⁺ (g) + e⁻ ΔH° = 1450kJ

F(g) + e⁻ → F⁻(g) ΔH° = -328kJ

Mg(s) + F₂(g) → MgF₂(s) ΔH° = -1123KJ

(Reaction is reversed and the sign of ∆Hº changed.)  

MgF2 (s) → Mg2+(g) + 2F–(g)            

2962 kJ

As ion charge rises, lattice energy rises as well. The lattice energy increases as the ion charge variable is increased. Accordingly, ions with higher charge intensities will result in ionic compounds with higher lattice energies.

Learn more about lattice energy here:

brainly.com/question/18222315

#SPJ4

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(part 1 of 3) Copper reacts with silver nitrate through a single replacement. If 1.29 g of silver are produced from the reaction
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See explanation.

Explanation:

Hello there!

In this case, according to the described chemical reaction, we first write the corresponding equation to obtain:

Cu+2AgNO_3\rightarrow 2Ag+Cu(NO_3)_2

Thus, we proceed as follows:

Part 1 of 3: here, since the molar mass of silver and copper (II) nitrate are 107.87 and 187.55 g/mol respectively, and the mole ratio of the former to the latter is 2:1, we can set up the following stoichiometric expression:

m_{Cu(NO_3)_2}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{1molCu(NO_3)_2}{2molAg}*\frac{187.55gCu(NO_3)_2}{1molCu(NO_3)_2}   \\\\m_{Cu(NO_3)_2}=1.12gCu(NO_3)_2

Part 2 of 3: here, the molar mass of copper is 63.55 g/mol and the mole ratio of silver to copper is 2:1, the mass of the former that was used to start the reaction was:

m_{Cu}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{1molCu}{2molAg}*\frac{63.55gCu)_2}{1molCu}   \\\\m_{Cu}=0.380gCu

Part 3 of 3: here, the molar mass of silver nitrate is 169.87 g/mol and their mole ratio 2:2, thus, the mass of initial silver nitrate is:

m_{AgNO_3}=1.29gAg*\frac{1molAg}{107.87gAg}*\frac{2molAgNO_3}{2molAg}*\frac{169.87gAgNO_3}{1molAgNO_3}   \\\\m_{AgNO_3}=2.03gAgNO_3

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