What are the 3 types of minerals?

A rigid 3.80 L sealed vessel contains 0.650 mol Ne, 0.321 mol Kr, and 0.190 mol Xe. Find the density of the mixture in g/L.

Eddi Din [679]

Answer:

17.09g/L

Explanation:

Density = total mass of elements/ volume

We need to find the mass of each mixture constituents using their molar mass:

mole = mass/molar mass

For Neon (Ne) which contains 0.650mol;

0.650 = mass/20.18

mass = 0.650 × 20.18

mass = 13.12g

For Krypton (Kr) which contains 0.321mol;

0.321 = mass/83.79

mass = 0.321 × 83.79

mass = 26.89g

For Xenon (Xe) which contains 0.190mol;

0.190 = mass/131.3

mass = 0.190 × 131.3

mass = 24.95g

Total mass = 13.12g + 26.89g + 24.95g = 64.96g

Density = total mass / volume

Density = 64.96g / 3.80L

Density of the mixture = 17.09g/L

7 0

3 years ago

2. What is the volume of 40.0 g of N2 at STP?

vampirchik [111]

Answer:

Molar mass of

N

2

=

28 g/mol

Moles of

40.5 g N

2

gas

=

40.5 g

28 g/mol

=

1.45 mol

1 mol

of any gas at

STP

occupies

22.4 L

of volume.

1.45 mol

of

N

2

gas will occupy

1.45

mol

×

22.4 L

1

mol

=

32.48 L

3 0

2 years ago

The reaction SO3 1g2 1 H2O1l2 h H2SO4 1AQ2 is the last step in the commercial production of sulfuric acid. the enthalpy change f

Phoenix [80]

Answer:

Cooling

Explanation:

Now, what we know is that the reaction would be exothermic. This knowledge is extractable in two ways. We know quite well that heat is released to the environment or surroundings and also the value of the enthalpy is negative. Thus we conclude that the reaction is exothermic.

Now, since heat is released to the environment, there is the need for an apparatus that would cool down the increased surrounding temperature. Hence, we can conclude that what we need actually is to provide cooling for the reaction mixture

7 0

3 years ago

The mystery of the unknown substance A prominent automotive businessman has been murdered in New York. The Crime Scene Investiga

Alisiya [41]

Data:

1) molar mass: 58.0714 g.

2) mass analysis

C: 18 g
H: 3 g
O: 8 g.

Solution

What is the percent composition of all the components in the liquid?

mass of C + mass of H + mass of O = 18g + 3g + 8g = 29 g

Percent composition:

C: (18g / 29g) * 100 = 62%

H: (3g / 29g) * 100 = 10%

O: (8g / 29g) * 100 = 28%
--------------
Total 100%

What is the empirical formula of the compound?

Convert masses to number of moles by dividing each mass by the atomic mass of the correspondant element:

C: 18 g/ 12.0 g/mol = 1.5 mol

H: 3 g / 1.0 g/mol = 3 mol

O: 8 g / 16 g/mol = 0.5 mol

Divide each number of moles by the smaller, i.e. 0.5 mol

=> C: 1.5 mol / 0.5 mol = 3 mol
=> H: 3 mol / 0.5 mol = 6 mol
=> O: 0.5 mol / o.5 mol = 1 mol

=> Empirical formula: C3 H6 O

What is the molecular formula of the unknown liquid?

First,calculate the molar mass of the empirical formula:

C3 H6 O => 3 * 12 g/mol + 6*1 g/mol + 16 g/mol = 58 g/ mol

Secont, given that the molar mass is the same that the empirical mass, the molecular formula is the same empirical formula.

=> Molecular formula = C3 H6 O.

This compound has been identified as a ketone.

Go online and figure out the name of this compound.

It is easy to find that this compound is propanone or acetone (both names are valid).

Now you can go online and find its characteristics and common uses.

Can you identify the killer from this information? How?

Likely they think you can presume that the killer is the actress, because women use acetone regularlty to remove the nail polish.

8 0

4 years ago

An air compressor draws in 1,200 cf of free air at a gauge pressure of 0 psi and a temperature of 70°F. The air is compressed to

lubasha [3.4K]

Answer:

The final volume of air after compression: V₂ = 4477.63 L = 158.12 cf

Explanation:

Given: Initial gauge pressure of the gas = 0 psi

Initial absolute pressure of the gas: P₁ = gauge pressure + atmospheric pressure = 0 psi + 12.20 psi = 12.20 psi

Initial Temperature = 70°F

⇒ T₁ = (70°F − 32) × 5/9 + 273.15 = 294.26 K

Initial volume of the gas: V₁ = 1200 cf = 1200 × 28.317 = 33980.4 L (∵ 1 cf ≈ 28.317 L)

Final gauge pressure of the gas = 90 psi

Final absolute pressure of the gas: P₂ = gauge pressure + atmospheric pressure = 90 psi + 12.20 psi = 102.2 psi

Final Temperature: T₂ = 125°F

⇒ T₂ = (125°F − 32) × 5/9 + 273.15 = 324.82 K

Final volume of the gas: V₂ = ? L

According to the Combined gas law:

$\frac{P_{1}\times V_{1}}{T_{1}} = \frac{P_{2}\times V_{2}}{T_{2}}$

→ $V_{2} = \frac{P_{1}\times V_{1}\times T_{2}}{T_{1}\times P_{2}}$

→ $V_{2} = \frac{12.20 psi\times 33980.4 L\times 324.82 K}{294.26 K\times 102.2 psi}$

→ $V_{2} = 4477.63 L = 158.12 cf$

Therefore, the final volume of air after compression: V₂ = 4477.63 L = 158.12 cf

7 0

4 years ago