All categories

2 years ago

Nitrogen from a mixture of nitrogen and oxgen

Chemistry

2 answers:

Sphinxa [80]2 years ago

5 0

Answer:

Explanation:

The liquid nitrogen and oxygen are then separated by fractional distillation . The liquefied air is passed into the bottom of a fractionating column. Just as in the columns used to separate oil fractions , the column is warmer at the bottom than it is at the top.

vivado [14]2 years ago

3 0

Oxygen - nitrogen gas mixture is a colorless odorless gas. Both oxygen and nitrogen are noncombustible; however, oxygen can accelerate the burning of a fire. Under prolonged exposure to fire or intense heat the containers may rupture violently and rocket.

You might be interested in

74) A solution is prepared by dissolving 0.60 g of nicotine (a nonelectrolyte) in water to make 12 mL of solution. The osmotic p

dusya [7]

Answer:

molar mass of nicotine will be 162.16g/mol

Explanation:

The mass of nicotine taken = 0.60g

The volume of solution = 12mL

the osmotic pressure of solution = 7.55 atm

Temperature in kelvin =298.15K (25+ 273.15)

The formula which relates osmotic pressure and concentration (moles per L) is:

π = MRT

Where

π = osmotic pressure (unit atm) = 7.55 atm

M = molarity (mol /L)

T= temperature = (K) = 298.15 K

R = gas constant = 0.0821 L atm /mol K

Putting values

$7.55=MX0.0821X298.15$

Therefore

$M=\frac{7.55}{0.0821X298.15}=0.308\frac{mol}{L}$

Molarity is moles of solute dissolve per litre of solution

The volume of solution in litre = 0.012 L

$molarity=\frac{moles}{V}$

$moles=molarityXvolume=0.308X0.012=0.0037mol$

we know that

$moles=\frac{mass}{ymolarmass}$

molar mass = $\frac{mass}{moles}=\frac{0.60}{0.0037}=162.16\frac{g}{mol}$

5 0

3 years ago

Name gaseous element in period 2 group 16?

Sholpan [36]

Answer:

mark me as a brainlist answer

Explanation:

Oxygen

3 0

2 years ago

Recovery standards are a necessary tool for determining exactly how much of a particular analyte you are able to extract from a

Dafna11 [192]

Answer:

2.05mg Fe/ g sample

Explanation:

In all chemical extractions you lose analyte. Recovery standards are a way to know how many analyte you lose.

In the problem you recover 3.5mg Fe / 1.0101g sample: 3.465mg Fe / g sample. As real concentration of the standard is 4.0 mg / g of sample the percent of recovery extraction is:

3.465 / 4×100 = 86,6%

As the recovery of your sample was 1.7mg Fe / 0.9582g, the Iron present in your sample is:

1.7mg Fe / 0.9582g sample× (100/86.6) = 2.05mg Fe / g sample

I hope it helps!

5 0

3 years ago

All of the food that we eat, liquids that we drink and medications that we take are

kirill115 [55]

A) Chemicals

(I'm pretty sure)

3 0

3 years ago

An atom can act as a tiny magnet due to the spinning motion of charged particles called neutrons. Please select the best answer

Tatiana [17]

Falso porque los neutrones no tienen carga

7 0

3 years ago