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Ann [662]
3 years ago
14

Nitrogen from a mixture of nitrogen and oxgen

Chemistry
2 answers:
Sphinxa [80]3 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]3 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.

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Milk of magnesia has the chemical formula Mg(OH)2. What is the mass of 3.2 moles of milk of magnesia? The molar Mass of magnesiu
GenaCL600 [577]
To calculate the mass of milk of magnesia given, we need certain data like molar mass of the compound which needs the atomic mass of the atoms in the compound. We calculate as follows:

Molar mass of <span>Mg(OH)2 = 24.3 g/mol + (2 x (16 + 1.0)) = 58.30 g/mol

Mass = 3.2 mol (</span>58.30 g/mol) = 186.56 grams
3 0
3 years ago
What is the mass of the solid NH4Cl formed when 75.5 g of NH3 is mixed with an equal mass of HCl? What is the volume of the gas
Gekata [30.6K]

Answer : The volume of the gas remaining is 56.5 liters.

The gas is hydrochloric acid and the formula of the gas is HCl.

The mass of NH_4Cl produced is, 110.7 grams.

Explanation :

The balanced chemical reaction will be:

NH_3+HCl\rightarrow NH_4Cl

First we have to calculate the moles of NH_3 and HCl

\text{Moles of }NH_3=\frac{\text{Mass of }NH_3}{\text{Molar mass of }NH_3}

Molar mass of NH_3 = 17 g/mole

\text{Moles of }NH_3=\frac{75.5g}{17g/mole}=4.44mole

and,

\text{Moles of }HCl=\frac{\text{Mass of }HCl}{\text{Molar mass of }HCl}

Molar mass of HCl = 36.5 g/mole

\text{Moles of }HCl=\frac{75.5g}{36.5g/mole}=2.07mole

Now we have to calculate the limiting and excess reagent.

From the balanced reaction we conclude that

As, 1 mole of HCl react with 1 mole of NH_3

So, 2.07 mole of HCl react with 2.07 mole of NH_3

From this we conclude that, NH_3 is an excess reagent because the given moles are greater than the required moles and HCl is a limiting reagent and it limits the formation of product.

The remaining moles of HCl gas = 4.44 - 2.07 = 2.37 moles

Now we have to calculate the volume of the gas remaining.

Using ideal gas equation :

PV = nRT

where,

P = Pressure of gas = 752 mmHg = 0.989 atm     (1 atm = 760 mmHg)

V = Volume of gas = ?

n = number of moles of gas = 2.37 moles

R = Gas constant = 0.0821 L.atm/mol.K

T = Temperature of gas = 14.0^oC=273+14.0=287K

Putting values in above equation, we get:

0.989atm\times V=2.37mole\times (0.0821L.atm/mol.K)\times 287K

V = 56.5 L

Now we have to calculate the moles of NH_4Cl

As, 1 mole of HCl react with 1 mole of NH_4Cl

So, 2.07 mole of HCl react with 2.07 mole of NH_4Cl

Now we have to calculate the mass of NH_4Cl

\text{ Mass of }NH_4Cl=\text{ Moles of }NH_4Cl\times \text{ Molar mass of }NH_4Cl

Molar mass of NH_4Cl = 53.5 g/mole

\text{ Mass of }NH_4Cl=(2.07moles)\times (53.5g/mole)=110.7g

Thus, the volume of the gas remaining is 56.5 liters.

The gas is hydrochloric acid and the formula of the gas is HCl.

The mass of NH_4Cl produced is, 110.7 grams.

3 0
3 years ago
The pen on seismograph swings freely.
Sever21 [200]
This statment is false, the pen on a seismograph does not swing freely.
7 0
3 years ago
What is the mass of 0.100 mole of neon? (Watch sf’s)
dimaraw [331]

Answer:

The answer to your question is letter D. 2.02 g

Explanation:

Data

moles of Ne = 0.100

atomic mass of Neon = 20.18 g

Process

1.- Use proportions to find the answer

                   20.18 g of Ne ------------------  1 mol of Ne

                        x                 ------------------  0.1 moles

                        x = (0.1 x 20.18)/1

                        x = 2.018

2.- Consider the significant figures

      0.100 has three significant figures so the answer must be  2.02 g

4 0
3 years ago
Read 2 more answers
Calculate the equilibrium constant of the reaction below if the pressures are 1.0atm, 2.0 atm, and 1.0 atm respectively. PCl3 +
Makovka662 [10]

Answer:

K = 0.5

Explanation:

Based on the reaction:

PCl₃ + Cl₂ ⇄ PCl₅

The equilibrium constant, K, is defined as:

K = P PCl₅ / P PCl₃ * P Cl₂

<em>Where P represent the pressure at the equilibrium for each one of the gases involved in the equilibrium.</em>

<em />

As:

P PCl₅ = 1.0atm

P PCl₃ = 1.0atm

P Cl₂ = 2.0atm

K = 1.0atm / 1.0atm * 2.0atm

<h3>K = 0.5</h3>
7 0
2 years ago
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