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2 years ago

Use the following to calculate ΔH°latice of MgF₂:

1 answer:

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:

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The standard enthalpy of formation (ΔHf°) of calcium carbonate is –1207 kJ/mol. Which ONE of the equations below has ΔH° = –1207

Art [367]

Answer:

A) Ca(s) + C(s) + 3/2 O₂(g) → CaCO₃(s)

Explanation:

Standard enthalpy of formation of a chemical is defined as the change in enthalpy durin the formation of 1 mole of the substance from its constituent elements in their standard states.

The consituent elements of calcium carbonate, CaCO₃, in their standard states (States you will find this pure elements in nature), are:

Ca(s), C(s) and O₂(g)

That means, the equation that represents standard enthalpy of CaCO₃ is:

<em>Is the equation that has ΔH° = -1207kJ/mol</em>

3 0

3 years ago

PLEASE HELP!!

Neporo4naja [7]

Fermentation
got it right on the test :)

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2 years ago

Starting with 2.50 mol of N2 gas (assumed to be ideal) in a cylinder at 1.00 atm and 20.0C, a chemist first heats the gas at con

arsen [322]

Answer:

a) $T_b=590.775k$

b) $W_t=1.08*10^4J$

d) $Q=3.778*10^4J$

d) $\triangle V=4.058*10^4J$

Explanation:

From the question we are told that:

Moles of N2 $n=2.50$

Atmospheric pressure $P=100atm$

Temperature $t=20 \textdegree C$

$t = 20+273$

$t = 293k$

Initial heat $Q=1.36 * 10^4 J$

Generally the equation for change in temperature is mathematically given by

$\triangle T=\frac{Q}{N*C_v}$

Where

$C_v=Heat\ Capacity \approx 20.76 J/mol/K$

$T_b-T_a=\frac{1.36 * 10^4 J}{2.5*20.76 }$

$T_b-293k=297.775$

$T_b=590.775k$

Generally the equation for ideal gas is mathematically given by

$PV=nRT$

For v double

$T_c=2*590.775k$

$T_c=1181.55k$

Therefore

$PV=Wbc$

$Wbc=(2.20)(8.314)(1181_590.778)$

$Wbc=10805.7J$

Total Work-done $W_t$

$W_t=Wab+Wbc$

$W_t=0+1.08*10^4$

$W_t=1.08*10^4J$

Generally the equation for amount of heat added is mathematically given by

$Q=nC_p\triangle T$

$Q=2.20*2907*(1181.55-590.775)\\$

$Q=3.778*10^4J$

Generally the equation for change in internal energy of the gas is mathematically given by

$\triangle V=nC_v \triangle T$

$\triangle V=2.20*20.76*(1181.55-293)k$

$\triangle V=4.058*10^4J$

3 0

3 years ago

Gemiola [76]

Answer:

the physical and chemical properties of the products are different from the reactants

Explanation:

A chemical reaction involves the chemical combination of two or more elements/compounds called Reactants to give one or more different elements/compounds called Products. A chemical reaction occurs in such a way that the atoms of the reactants are restructured to form product(s) that is/are entirely different from the reactants.

In a chemical reaction, the physical and chemical properties of the products differ from that of the reactants since different chemical compounds/elements are formed as products. The physical properties of a substance, which include colour, melting and boiling point etc. will differ in the reactants and products formed. Also, the chemical structure and identity of the reactants will be changed to give rise to a different chemical property in the products.

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3 years ago

What is the heat of reaction (AH) of the<br> following?<br> C(s) + O2 (g) --> CO2 (g)

zlopas [31]

Answer:

C co2 2co enthalpy

2 Answers. Ernest Z. The standard enthalpy of formation of carbon monoxide is -99 kJ/mol.

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3 years ago