How can some of the difficulties caused by the Down Syndrome be over come?

A compound with molecular formula C6H15N exhibits a singlet at d 0.9 ppm (1H), a triplet at 1.10 ppm (3H), a singlet at 1.15 ppm

Triss [41]

Answer:

CH3 - CH2 - NH - C(CH3)3

Explanation:

The 1HNMR is the acronym for Proton nuclear magnetic resonance and it is used in chemistry or Chemical laboratory for the analysis and identification of compounds.

In order to be able to answer the question accurately you have to have the tables containing all the values for chemical shift. The Chemical shift is measured in ppm and it occur due to Resonance frequency variation.

From the table, a singlet at 1.15 ppm (9H) is - C(CH3)3.

A singlet at d 0.9 ppm (1H) shows the presence of a secondary amine group, that is -R2NH group.

A triplet at 1.10 ppm (3H) shows that we have;

CH3- CH2-

A quartet at 2.6 ppm (2H) shows that we have;

-CH2 - CH3.

Therefore, joining all together we have;

CH3 - CH2 - NH - C(CH3)3.

Kindly check attached file for the picture of the structure.

5 0

2 years ago

Which is the correct formula for the compound made when aqueous solutions containing a dissolved magnesium compound and a dissol

jenyasd209 [6]

It would be MgCl₂ ~ Magnesium Chloride.

4 0

3 years ago

Read 2 more answers

A sample of water is heated from 60.0 °C to 75.0°C by the addition of 140 j of

kupik [55]

Mass of the water : 2.23 g

<h3>Furter explanation</h3>

Heat

Q = m.c.Δt

m= mass, g

c = heat capacity, for water : 4.18 J/g° C.

ΔT = temperature

Q= 140 J

Δt = 75 - 60 = 15

mass of the water :

$\tt m=\dfrac{Q}{c.\Delta T}=\dfrac{140}{4.18\times 15}=2.23~g$

5 0

2 years ago

What volume of so2 is produced at 325 k and 1.35 atm when 15.0 grams of hcl reacts with excess k2so3?

Helen [10]

The balanced equation for the above reaction is as follows;
2HCl + K₂SO₃ ---> 2KCl + H₂O + SO₂
stoichiometry of HCl to SO₂ is 2:1
number of moles of HCl reacted - 15.0 g / 36.5 g/mol = 0.411 mol
according to molar ratio
number of SO₂ moles formed - 0.411 mol /2 = 0.206 mol
since we know the number of moles we can find volume using ideal gas law equation
PV = nRT
where
P - pressure - 1.35 atm x 101 325 Pa/atm = 136 789 Pa
V - volume
n - number of moles - 0.206 mol
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature - 325 K
substituting values in the equation

136 789 Pa x V = 0.206 mol x 8.314 Jmol⁻¹K⁻¹ x 325 K
V = 4.07 L
volume of SO₂ formed is 4.07 L

8 0

3 years ago

Assuming that a tank of gasoline contains 80 liters and that its density is 0.77 kg/liter, determine how many kg of co2 are prod

sleet_krkn [62]

Answer: -

If a tank of gasoline contains 80 liters and that its density is 0.77 kg/liter, 0.26 kg of CO₂ are produced for each tank of gasoline burned.

Explanation: -

Density of the gasoline = 0.77 kg / liter

Volume of the tank containing the gasoline = 80 liter.

Mass of gasoline produced from each tank

= Volume of the tank containing the gasoline x Density of the gasoline

= $\frac{0.77 kg}{1 liter}$ x 80 liter

= 61.6 kg

Chemical formula of gasoline = C₈H₁₈

Molar mass of gasoline C₈H₁₈ = 12 x 8 + 1 x 18 = 114 g/ mol

Number of moles of C₈H₁₈ = $\frac{61.6 g}{114 g}$ x 1 mol

= 0.54 mol of C₈H₁₈

The chemical equation for the burning of gasoline is

2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

From the balanced equation we see

2 mol of C₈H₁₈ gives 16 mol of CO₂

0.54 mol of C₈H₁₈ gives $\frac{16 mol CO2 x 0.54 mol C8H18}{2 mol C8H18}$ mol of CO₂

= 4.32 mol of CO₂

Molar mass of CO₂ = 12 x 1 + 16 x 3 =60 g / mol

Mass of CO₂ = Molar mass of CO₂ x Number of moles of CO₂

= $\frac{60g x 4.32 mol}{1 mol}$

= 259.2 g

= $\frac{259.2}{1000}$

= 0.259 Kg

= 0.26 kg rounded off to 2 significant figures.

Thus if a tank of gasoline contains 80 liters and that its density is 0.77 kg/liter, 0.26 kg of CO₂ are produced for each tank of gasoline burned.

4 0

3 years ago