Ask question

Ask question

All categories

3 years ago

14

Under what conditions does the molar volume of a gas decrease

2 answers:

aalyn [17]3 years ago

5 0

The volume decreases in the same ratio as the ratio of pressure increases. But you won't get any change in volume.

nydimaria [60]3 years ago

4 0

Answer:

Gases are compressible, meaning that when put under high pressure, the particles are forced closer to one another. This decreases the amount of empty space and reduces the volume of the gas. Gas volume is also affected by temperature. When a gas is heated, its molecules move faster and the gas expands.

You might be interested in

Treatment of 2-hexanone with naoch2ch3 followed by ch3br affords compound x (c7h14o) as the major product. x shows a strong abso

VashaNatasha [74]

The given ketone when reacted with base gave enolate, the enolate formed due to loss of methylene proton next to carbonyl group. Enolate when treated with methyle Bromide gave alpha substituted product.

Strong absorption around 1713 cm⁻¹ in IR spectrum confirms the presence of Carbonyl group.

The product along with ¹H-NMR values is given below,

8 0

4 years ago

Some plants can grow from both blank and blank

LUCKY_DIMON [66]

Plants can grow from sunlight and water.

3 0

3 years ago

Read 2 more answers

1) How many molecules are there in 985 mL of nitrogen at 0.0° C and 1.00 x 10-6 mm Hg?

RSB [31]

Answer : The number of molecules present in nitrogen gas are, $3.48\times 10^{13}$

Explanation :

First we have to calculate the moles of nitrogen gas by using ideal gas equation.

$PV=nRT$

where,

P = Pressure of $N_2$ gas = $1.00\times 10^{-6}mmHg=1.32\times 10^{-9}atm$ (1 atm = 760 mmHg)

V = Volume of $N_2$ gas = 985 mL = 0.982 L (1 L = 1000 mL)

n = number of moles $N_2$ = ?

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

T = Temperature of $N_2$ gas = $0.0^oC=273+0.0=273K$

Now put all the given values in above equation, we get:

$(1.32\times 10^{-9}atm)\times 0.982L=n\times (0.0821L.atm/mol.K)\times 273K$

$n=5.78\times 10^{-11}mol$

Now we have to calculate the number of molecules present in nitrogen gas.

As we know that 1 mole of substance contains $6.022\times 10^{23}$ number of molecules.

As, 1 mole of $N_2$ gas contains $6.022\times 10^{23}$ number of molecules

So, $5.78\times 10^{-11}$ mole of $N_2$ gas contains $(5.78\times 10^{-11})\times (6.022\times 10^{23})=3.48\times 10^{13}$ number of molecules

Therefore, the number of molecules present in nitrogen gas are, $3.48\times 10^{13}$

8 0

3 years ago

Please help and if u dont know that ok but pleas don't give me the wrong answer

Levart [38]

Answer: The answer is 2 and 4

6 0

3 years ago

Read 2 more answers

What is the number of orbitals in an atom of radon

yan [13]

86 elections so 43 orbitals

6 0

3 years ago