Which is the correct Lewis dot structure of NH2? A.A B.B C.C D.D E.E

Separate this redox reaction into its component half-reactions. 3o2 4co

swat32

The equation is:
3 O₂ + 4 Co → 2 Co₂O₃
Oxidation half reaction:
Co → Co³⁺ + 3 e
Reduction half reaction:
O₂ + 4 e → 2 O²⁻
To balance the equation number of electrons lost must be equal to number or electrons gained so we must multiply oxidation half time 4 and reduction half times 3

3 0

3 years ago

PLEASE HELP ME ASAP!!!!!!!!!

snow_lady [41]

Answer:

the answer is c 8.91g/cm³

6 0

3 years ago

ILL GIVE BRAINLIST............ have to answer all!!!!

7nadin3 [17]

1 is seconds and meters m/s

2 is seconds and meters m/s^2

3 Newton kg/m

4 Kilograms

Hope this helps!

6 0

3 years ago

Use the following data to estimate ΔHf° for magnesium fluoride. Mg(s) + F2(g) → MgF2(s) lattice energy −2913 kJ/mol first ioniza

miss Akunina [59]

Answer:

The correct answer is -1085 KJ/mol

Explanation:

To calculate the formation enthalphy of a compound by knowing its lattice energy, you have to draw the Born-Haber cycle step by step until you obtain each element in its gaseous ions. Find attached the correspondent Born-Haber cycle.

In the cycle, Mg(s) is sublimated (ΔHsub= 150 KJ/mol) to Mg(g) and then atoms are ionizated twice (first ionization: ΔH1PI= 735 KJ/mol, second ionization= 1445 KJ/mol) to give the magnesium ions in gaseous state.

By other hand, the covalent bonds in F₂(g) are broken into 2 F(g) (Edis= 154 KJ/mol) and then they are ionizated to give the fluor ions in gaseous state 2 F⁻(g) (2 x ΔHafinity=-328 KJ/mol). The ions together form the solid by lattice energy (ΔElat=-2913 KJ/mol).

The formation enthalphy of MgF₂ is:

ΔHºf= ΔHsub + Edis + ΔH1PI + ΔH2PI + (2 x ΔHaffinity) + ΔElat

ΔHºf= 150 KJ/mol + 154 KJ/mol + 735 KJ/mol + 1445 KJ/mol + (2 x (-328 KJ/mol) + (-2913 KJ/mol).

ΔHºf= -1085 KJ/mol