Indicate type of chemical reactions for 2Mgl2+MN(SO3)2=2MgSO3+Mnl4<br>

P4 (s) + 5O2 (g) ⟶ P4 O10(s) ΔG° = −2697.0 kJ/mol 2H2 (g) + O2 (g) ⟶ 2H2 O(g) ΔG° = −457.18 kJ/mol 6H2 O(g) + P4 O10(s) ⟶ 4H3 PO

aalyn [17]

Answer:

the standard free energy of formation of phosphoric acid H3 PO4 is -1010 kJ/mol

Explanation:

Knowing that

1) P4 (s) + 5O2 (g) ⟶ P4 O10(s) ΔG° = −2697.0 kJ/mol

2) 2H2 (g) + O2 (g) ⟶ 2H2 O(g) ΔG° = −457.18 kJ/mol

3) 6H2 O(g) + P4 O10(s) ⟶ 4H3 PO4 (l) ΔG° = −428.66 kJ/mol

since

ΔG° reaction = ν * ΔGf ° products - v *ΔGf ° reactives

for reaction 1

ΔG° = ∑ν * ΔGf ° products - ∑v *ΔGf ° reactives

ΔG° = 1 *ΔGf ° P4 O10 - ( 5 *ΔGf ° O2 + 1 *ΔGf ° P4)

ΔG° = ΔGf ° P4 O10 - (5*0 +1*0)

ΔGf ° P4 O10 = ΔG° = −2697.0 kJ/mol

for reaction 2

ΔG° = ∑ν * ΔGf ° products - ∑v *ΔGf ° reactives

ΔG° = 2 *ΔGf ° H20 - ( 1*ΔGf ° O2 + 2 *ΔGf ° H2)

ΔG° = 2* ΔGf ° H20 - (1*0 +2*0)

ΔGf ° H20 = ΔG° /2 = -457.18 kJ/mol/2 = -228.59 kJ/mol

for reaction 3

ΔG° = ∑ν * ΔGf ° products - ∑v *ΔGf ° reactives

ΔG° = 4 *ΔGf ° H3 PO4 - ( 6*ΔGf ° H2O + 1*ΔGf ° P4O10)

−428.66 kJ/mol = 4 *ΔGf ° H3 PO4 - [ 6*(-228.59 kJ/mol) + 1*(−2697.0 kJ/mol)]

−428.66 kJ/mol = 4 *ΔGf ° H3 PO4 + 3611.36 kJ/mol

ΔGf ° H3 PO4 = (−428.66 kJ/mol - 3611.36 kJ/mol)/4 = -1010 kJ/mol

6 0

3 years ago

Please check my answer! Due in a few minutes!

rewona [7]

Answer:

Explanation:

It is A. that is the only one that really makes any sense to me.

I do hope I helped you! :)

8 0

3 years ago

Read 2 more answers

Fluorine (F) and bromine (Br) are in the same group on the periodic table. How do atoms of these elements compare when they form

sertanlavr [38]

Answer:

Both a fluorine atom and a bromine atom gain one electron, and both atoms become stable.

Explanation:

The two elements compare when they form bonds in that when both a fluorine atom and a bromine atom gain one electron, they both become stable.

Fluorine and bromine are elements called halogens.
They both belong to group 7 on the periodic table.
When they gain an electron each, they become isoelectronic with a corresponding noble gas.
This gives their atom special stability.

3 0

3 years ago

Read 2 more answers

Which of the following reactions is correctly balanced?

Kitty [74]

I believe it is 3 CA + 1 N2 -> Ca3N2; I cannot tell whether the O(s) in front of the next three are supposed to be oxygens, if so then yes definitely the first line is correctly balanced.

7 0

3 years ago

The information below describes a redox reaction.

Vera_Pavlovna [14]

3

Explanation:

The coefficient in the final, balanced equation for the reaction is 3.

Now let us look into the reaction:

The half equations are;

Ag⁺ + e⁻ → Ag reduction half

Al → Al³⁺ + 3e⁻ oxidation half

The reduction half, electron is taken in where as in the oxidation half, electron is lost.

To derive the over all balanced equation;

Ag⁺ + e⁻ → Ag multiply by 3

Al → Al³⁺ + 3e⁻ multiply by 1

This gives :

3Ag⁺ + 3e⁻ → 3Ag

Al → Al³⁺ + 3e⁻

Adding reactants together and products together:

3Ag⁺ + 3e⁻ + Al → 3Ag + Al³⁺ + 3e⁻

Cancel out species that appears on both sides of the expression because they are spectators:

3Ag⁺ $_{aq}$ + Al $_{s}$ → 3Ag $_{s}$ + Al³⁺ $_{aq}$

We see that silver has a coefficient of 3 in the balanced expression.

learn more:

Ionic equation brainly.com/question/2947744

#learnwithBrainly

6 0

4 years ago

Indicate type of chemical reactions for 2Mgl2+MN(SO3)2=2MgSO3+Mnl4​

Indicate type of chemical reactions for 2Mgl2+MN(SO3)2=2MgSO3+Mnl4