Which is a diatomic molecule? A. Ar B. CO C. CO2 D. NaCl

Calculate the specific volume of Helium using the compressibility factor. 500 kPa, 60 degrees Celsius

IrinaK [193]

Explanation:

Formula for compressibility factor is as follows.

z = $\frac{P \times V_{m}}{R \times T}$

where, z = compressibility factor for helium = 1.0005

P = pressure

$V_{m}$ = molar volume

R = gas constant = 8.31 J/mol.K

T = temperature

So, calculate the molar volume as follows.

$V_{m} = \frac{z \times R \times T}{P}$

= $\frac{1.0005 \times 8.314 \times 10^{-3} m^{3}.kPa/mol K \times (60 + 273)K}{500 kPa}$

= 0.0056 $m^{3}/mol$

As molar mass of helium is 4 g/mol. Hence, calculate specific volume of helium as follows.

$V_{sp} = \frac{V_{m}}{M_{w}}$

= $\frac{0.0056 m^{3}/mol}{4 g/mol}$

= 0.00139 $m^{3}/g$

= 0.00139 $m^{3}/g \times \frac{1 g}{10^{-3}kg}$

= 1.39 $m^{3}/kg$

Thus, we can conclude that the specific volume of Helium in given conditions is 1.39 $m^{3}/kg$ .

7 0

3 years ago

Rank and explain how the freezing point of 0.100 m solutions of the following ionic electrolytes compare. List from lowest freez

Elden [556K]

Answer:

The solutions are listed from the lowest freezing point to highest freezing point.

Mg₃(PO₄)₂ - AlBr₃ - BeBr₂ - KBr

Explanation:

Colligative property of freezing point, is the freezing point depression.

Formula is:

ΔT = Kf . m . i

Where ΔT = T° freezing pure solvent - T° freezing solution

Kf is the cryoscopic constant

m is molality and i is the Van't Hoff factor (number of ions, dissolved in solution)

In this case, T° freezing pure solvent is 0° because it's water, so the Kf is 1.86 °C/m, and m is 0.1 molal.

The i modifies the T° freezing solution. The four salts, are ionic compounds, so for each case:

BeBr₂ → Be²⁺ + 2Br⁻ i = 3

AlBr₃ → Al³⁺ + 3Br⁻ i = 4

Mg₃(PO₄)₂ → 3Mg²⁺ + 2PO₄⁻³ i = 5

KBr → K⁺ + Br⁻ i = 2

Solution of Mg₃(PO₄)₂ will have the lowest temperature of freezing and the solution of KBr, the highest (always lower, than 0°).

8 0

3 years ago

Which of the following statements is not correct?

Pavlova-9 [17]

Answer: This option is incorrect: B. Covalent compounds are held together by much stronger interparticle forces than are ionic compounds.

Justification:

Ionic bonds, held by ionic compounds, are much stronger than covalent bonds, held by covalent compounds.

In ionic bonds one element yields one or more electrons forming a cation (a positively charged ion) and the other element accepts the electrons forming an anion (a negatively charged ion).

The anion and the cation are electrostatically atracted by each other. This electrostatic atraction force, named ionic bond, is very strong.

As result of this, the ionic compounds form strong crystals with high boiling and fusion points. A good example of this the sodium chloride, formed by the union of cation Na(+) and anion Cl(-).

The covalent bonds are result of sharing electrons and do not form ions. This bond is weaker than the ionic bond.

4 0

4 years ago

Which is true of a solute dissolved in a solvent? the solute raises the boiling point of the solvent. the solvent decreases the

Lina20 [59]

When a solute is dissolved in a solvent the solute raises the boiling point of the solvent. The boiling point of a liquid (a solvent) will be higher when another compound (solute) is added, such that a solution has a higher boiling point than a pure solvent. This takes place when a non-volatile solute, such as a salt, is added to a pure solvent such as water.

6 0

3 years ago

What changes in trade did Europeans hope to bring about by finding sea routes to Asian markets?

Dovator [93]

Answer:

controlled by the Arabs, who brought frankincense and myrrh by camel caravan from South Arabia.

3 0

3 years ago