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tangare [24]
3 years ago
14

Identify the reagents necessary to achieve each of the following transformations: Na2Cr2O7, H2SO4, H2O EtOH, H+ H2O Fe2+, NaOH N

a2Cr2O7, H2SO4, H2O PCC, CH2Cl2 H2O, H+ Fe2+, H+ 1) R2B-H 2) H2O2, NaOH H2SO4, H2O, HgSO4 1) Br2 2) KOH H2SO4, H2O 1) R2B-H 2) H2O2, NaOH H2SO4, H2O, HgSO4 H2SO4, H2O 1) Br2, KOH 2) H2O, H+ 1) O3 2) DMS 1) O2 2) DMS 1) Br2 2) KOH K2Cr2O7, H2SO4, H2O
Chemistry
1 answer:
Gala2k [10]3 years ago
8 0
There’s not an answer in there.
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What is the volume occupied by 4.20 miles of oxygen gas (O2) at STP
Drupady [299]

Answer: 94.13 L

Explanation: In STP in an ideal gas there is a standard value for both temperature and pressure. At STP,pressure is equal to 1atm and the temperature at 0°C is equal to 273.15K. This problem is an ideal gas so we use PV=nRT where R is a constant R= 0.08205 L.atm/mol.K.

To find volume, derive the equation, it becomes V=nRT/P. Substitute the values. V= 4.20 mol( 0.08205L.atm/mol.K)(273.15K) / 1 atm = 94.13 L. The mole units, atm and K will be cancelled out and L will be the remaining unit which is for volume.

8 0
2 years ago
Calculate the enthalpy of the formation of butane, C4H10, using the balanced chemical equation and the standard value below:
zavuch27 [327]

Answer:

+125.4 KJmol-1

Explanation:

∆H C4H10(g) = -2877.6kJ/mol

∆H C(s)=-393.5kJ/mol

∆H H2(g) = -285.8

∆H reaction= ∆Hproducts - ∆H reactants

∆H reaction= (-2877.6kJ/mol) - [4(-393.5kJ/mol) +5(-285.8)]

∆H reaction= +125.4 KJmol-1

6 0
3 years ago
Name three sources of CO2
dangina [55]

Answer:

1.Respiration of animals and plants.

2.The burning of fossil fuels.

3.Bacteria decompose corpses.

4 0
3 years ago
Read 2 more answers
What is the hardest mineral? <br> A. Feldspar <br> B. Fluorite<br> C. Galena<br> D. Quarts
Zinaida [17]
D it’s quartz on the Mohs scale thing it’s ranked 7
3 0
3 years ago
Due to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much less common and less s
steposvetlana [31]
We are told we have an oxyacid of the formula HOFO. We will assume the atoms are in this order and will draw a proper lewis structure for this compound by first drawing bonds between each of the 4 atoms and then place the remaining electron pairs on each atom:
      ..    ..    ..
H - O - F - O:
      ··   ··    ··
We can calculate the formal charge of an atom using the following formula:

Formal charge = [# of valence electrons] - [# of non-bonded electrons + # of bonds]

H: Formal charge = [1]-[0+1] = 0

O: Formal charge = [6]-[4+2] = 0

F: Formal charge = [7]-[4+2] = +1

O: Formal charge = [6]-[6+1] = -1

As we can see the overall charge of the molecule is neutral since the fluorine as a +1 charge and the oxygen a -1 charge.
4 0
3 years ago
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