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BARSIC [14]
3 years ago
10

3) Ha do vapor aod gases differ?

Chemistry
1 answer:
Neko [114]3 years ago
6 0

Your question, I guess, How do vapour and gases differ...

Answer:

1.) Vapour is the changed state of any liquid either due to boiling or evaporation

2.) Vapour are more energetic as they have absorbed the latent heat of vaporization whereas Gases are low in energy because they are already in gaseous form at room temperature.

3.) Vapour have boiling points above room temperature while gases have their boiling point below room temperature.

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Which gas would have the slowest rate of diffusion, assuming that all gases are at the same temperature?
Iteru [2.4K]

Answer: radon (atomic mass 222 amu

Explanation:

To calculate the rate of diffusion of gas, we use Graham's Law.

This law states that the rate of effusion or diffusion of gas is inversely proportional to the square root of the molar mass of the gas. The equation given by this law follows:

\text{Rate of diffusion}\propto \frac{1}{\sqrt{\text{Molar mass of the gas}}}

atomic mass of krypton= 83.8 amu

atomic mass of argon= 39.95 amu

atomic mass of xenon = 131.3 amu

atomic mass of radon= 222 amu

Thus as atomic mass of radon is highest, its rate of diffusion is slowest.

7 0
3 years ago
Explain Newton's second law​
zhenek [66]

Answer:

The acceleration of an object as produced by a net force is directly proportional to the magnitude of the net force, in the same direction as the net force, and inversely proportional to the mass of the object

Explanation:

5 0
3 years ago
Read 2 more answers
PLEASE HELP!!
LUCKY_DIMON [66]

Answer:

5.1 - 2.3685 = 2.7315 \\

3 0
2 years ago
Using the standard enthalpies of formation found in the textbook, determine the enthalpy change for the combustion of ethanol c2
ArbitrLikvidat [17]
Enthalpy of formation is calculated by subtracting the total enthalpy of formation of the reactants from those of the products. This is called the HESS' LAW.
ΔHrxn = ΔH(products) - ΔH(reactants)

Since the enthalpies are not listed in this item, from reliable sources, the obtained enthalpies of formation are written below.
ΔH(C2H5OH) = -276 kJ/mol
ΔH(O2) = 0 (because O2 is a pure substance)
ΔH(CO2) = -393.5 kJ/mol
ΔH(H2O) = -285.5 kJ/mol

Using the equation above,
ΔHrxn = (2)(-393.5 kJ/mol) + (3)(-285.5 kJ/mol) - (-276 kJ/mol)
ΔHrxn = -1367.5 kJ/mol

<em>Answer: -1367.5 kJ/mol</em>
6 0
3 years ago
Read 2 more answers
Consider two equal-volume balloons under the same conditions of temperature and pressure. One contains helium, and the other con
Olegator [25]

Answer:

1. Number of gas particles (atoms or molecules)

2. Number of moles of gas

3. Average kinetic energy

Explanation:

Since the two gas has the same volume and are under the same conditions of temperature and pressure,

Then:

1. They have the same number of mole because 1 mole of any gas at stp occupies 22.4L. Now both gas will occupy the same volume because they have the same number of mole

2. Since they have the same number of mole, then they both contain the same number of molecules as explained by Avogadro's hypothesis which states that at the same temperature and pressure, 1 mole of any substance contains 6.02x10^23 molecules or atoms.

3. Being under the same conditions of temperature and pressure, they both have the same average kinetic energy. The kinetic energy of gas is directly proportional to the temperature. Now that both gas are under same temperature, their average kinetic energy are the same.

5 0
3 years ago
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