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antiseptic1488 [7]
3 years ago
13

PLEASE HELP ME ASAP!!! THIS IS DUE UNTIL 1:30 PM!!! Tell how many Elements are in this compound and tell what the Elements are.

NaClOFeCoH
Chemistry
2 answers:
il63 [147K]3 years ago
5 0

Answer:

6 elements

Explanation:

each element Na, Cl, O, Fe, Co, H

Nuetrik [128]3 years ago
4 0

Answer: 13

Explanation: I got it right

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The correct answer is A. The image shows a nuclear fission. This takes place in any of the heavy nuclei after capture of a neutron. This is the opposite of nuclear fusion. In this case, nuclei are broken down into two.
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3 years ago
The density of pentanol, C3H20, is 0.8110 g/mL. Calculate the volume occupied by 7.455 moles of pentanol. What is the volume occ
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Answer:

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Explanation:

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7 0
3 years ago
The following information was recorded by a student team working to prepare nickel sulfate. Plan: Prepare NiSO4 by reacting NiO
mixas84 [53]

Answer:

The options e and d are correct.

Explanation:

Mass of NiO = 7.5 g

Moles of NiO = \frac{7.5 g}{74.69 g/mol}=0.10 mol

Moles of sulfuric acid = n

Volume of sulfuric acid ,V= 50 mL = 0.050 L

Molarity of sulfuric acid ,M = 6 mol/L

n=M\time V=6mol/L\times 0.050 L =0.3 mol

NiO + H_2SO_4\rightarrow NiSO_4 + H_2O

According to reaction, 1 mole of NiO reacts with 1 mole of sulfuric acid.

Then 0.10 moles of NiO reacts with :

\frac{1}{1}\times 0.10 mol/=0.10 mol of sulfuric acid.

As we can see that sulfuric acid is in excess amount, so the amount of the product will depend upon amount of NiO.

According to reaction, 1 mole of NiO gives with 1 mole of NiSO_4.

Then 0.10 moles of NiO wil give :

\frac{1}{1}\times 0.10 mol/=0.10 mol of  NiSO_4.

Molar mass of  NiSO_4 = 154.75 g/mol

Mass of 0.10 moles of NiSO_4:

= 154.75 g/mol × 0.10 mol = 15.475 g

Theoretical mass of NiSO_4 = 15.475 g

Experimental yield of NiSO_4 = 17.4 g

Percentage yield :

\Yield=\frac{\text{Experimental mass}}{\text{Theoretical mass}}\times 100

Percentage yield of NiSO_4:

\Yield=\frac{17.4}{15.475 g}\times 100=112\%

Moles of NiSO_4.6H_2O = 262.85 g/mol × 0.10 mol = 26.285 g

Experimental yield of NiSO_4.6H_2O = 17.4 g

Percentage yield of NiSO_4.6H_2O:

\Yield=\frac{17.4}{26.285 g}\times 100=66.2\%

3 0
3 years ago
What is the relationship between the density and position of each Earth layer?
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Answer:

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Hope it helps

Please mark me as brainliest

THank you

6 0
2 years ago
Read 2 more answers
KFell Fe"(CN), + e + Nat → KNaFe'Fe(CN)6
Alinara [238K]

Answer:

Most common oxidation states: +2, +3

M.P. 1535º

B.P. 2750º

Density 7.87 g/cm3

Characteristics: Iron is a gray, moderately active metal.

Characteristic reactions of Fe²⁺ and Fe³⁺

The [Fe(H2O)6]3+ ion is colorless (or pale pink), but many solutions containing this ion are yellow or amber-colored because of hydrolysis. Iron in both oxidation states forms many complex ions.

Aqueous Ammonia

Aqueous ammonia reacts with Fe(II) ions to produce white gelatinous Fe(OH)2, which oxidizes to form red-brown Fe(OH)3:

Fe2+(aq)+2NH3(aq)+3H2O(l)↽−−⇀Fe(OH)2(s)+2NH+4(aq)(1)

Fe3appt.gif

Aqueous ammonia reacts with Fe(III) ions to produce red-brown Fe(OH)3:

Fe3+(aq)+3NH3(aq)+3H2O(l)↽−−⇀Fe(OH)3(s)+3NH+4(aq)(2)

Fe3bppt.gif

Both precipitates are insoluble in excess aqueous ammonia. Iron(II) hydroxide quickly oxidizes to Fe(OH)3 in the presence of air or other oxidizing agents.

Sodium Hydroxide

Sodium hydroxide also produces Fe(OH)2 and Fe(OH)3 from the corresponding oxidation states of iron in aqueous solution.

Fe2+(aq)+2OH−(aq)↽−−⇀Fe(OH)2(s)(3)

Fe4appt.gif

Fe3+(aq)+3OH−(aq)↽−−⇀Fe(OH)3(s)(4)

Fe4bppt.gif

Neither hydroxide precipitate dissolves in excess sodium hydroxide.

Potassium Ferrocyanide

Potassium ferrocyanide will react with Fe3+ solution to produce a dark blue precipitate called Prussian blue:

K+(aq)+Fe3+(aq)+[Fe(CN)6]4−(aq)↽−−⇀KFe[Fe(CN)6](s)(5)

Fe5a1ppt.gif

With Fe2+ solution, a white precipitate will be formed that will be converted to blue due to the oxidation by oxygen in air:

2Fe2+(aq)+[Fe(CN)6]4−(aq)↽−−⇀Fe2[Fe(CN)6](s)(6)

Fe5a2ppt.gif

Many metal ions form ferrocyanide precipitates, so potassium ferrocyanide is not a good reagent for separating metal ions. It is used more commonly as a confirmatory test.

Potassium Ferricyanide

Potassium ferricyanide will give a brown coloration but no precipitate with Fe3+. With Fe2+, a dark blue precipitate is formed. Although this precipitate is known as Turnbull's blue, it is identical with Prussian blue (from Equation 5).

K+(aq)+Fe+2(aq)+[Fe(CN)6]3−(aq)↽−−⇀KFe[Fe(CN)6](s)(7)

Fe5b.gif

Potassium Thiocyanate

KSCN will give a deep red coloration to solutions containing Fe3+:

Fe+3(aq)+NCS−(aq)↽−−⇀[FeNCS]+2(aq)(8)

Fe5cppt.gif

No Reaction

Cl−, SO2−4

7 0
3 years ago
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