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2 years ago

Help me please!

2 answers:

7 0

Ideal gas law is valid only for ideal gas not for vanderwaal gas. Therefore, the pressure that will be required for neon at 30°C to have the same density as nitrogen at 20°C and 1.0 atm is 1.44atm.

<h3>What is ideal gas equation?</h3>

Ideal gas equation is the mathematical expression that relates pressure volume and temperature. There is no force of attraction between the particles.

Mathematically the relation between Pressure and temperature can be given as

P₁M₁=DRT₁

P₂M₂=DRT₂

Rearranging the two equation we get

P₁M₁÷T₁=P₂M₂÷T₂

where,

P = pressure

M= Molarity

D=density

T =temperature

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

Substituting all the given values, we get

(P₁×M₁)÷T₁=(P₂×M₂)÷T₂

(P₁×20)÷303=(1.0 ×28)÷293

P₁=1.44atm

Therefore, the pressure that will be required for neon at 30°C to have the same density as nitrogen at 20°C and 1.0 atm is 1.44atm.

To learn more about ideal gas equation, here:

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Nataly_w [17]2 years ago

4 0

The pressure must be 1.03.

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3 years ago

A mixture of nitrogen and hydrogen gases, at a total pressure of 663 mm Hg, contains 3.46 grams of nitrogen and 0.156 grams of h

STALIN [3.7K]

Answer: The partial pressure of nitrogen gas is 405.76 mmHg and that of hydrogen gas is 257.24 mmHg

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

For nitrogen gas:

Given mass of nitrogen gas = 3.46 g

Molar mass of nitrogen gas = 28 g/mol

Putting values in above equation, we get:

$\text{Moles of nitrogen gas}=\frac{3.46g}{28g/mol}=0.123mol$

For hydrogen gas:

Given mass of hydrogen gas = 0.156 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in above equation, we get:

$\text{Moles of hydrogen gas}=\frac{0.156g}{2g/mol}=0.078mol$

Mole fraction of a gas is calculated by using the formula:

$\chi_{A}=\frac{n_{A}}{n_{A}+n_{B}}$ ......(1)

For nitrogen gas:

Putting values in equation 1, we get:

$\chi_{\text{nitrogen gas}}=\frac{0.123}{0.123+0.078}=0.612$

For hydrogen gas:

Putting values in equation 1, we get:

$\chi_{\text{hydrogen gas}}=\frac{0.078}{0.123+0.078}=0.388$

The partial pressure of a gas is given by Raoult's law, which is:

$p_A=p_T\times \chi_A$ ......(2)

where,

$p_A$ = partial pressure of substance A

$p_T$ = total pressure = 663 mmHg

$\chi_A$ = mole fraction of substance A

For nitrogen gas:

$p_{\text{Nitrogen gas}}=663mmHg\times 0.612\\\\p_{\text{Nitrogen gas}}=405.76mmHg$

For hydrogen gas:

$p_{\text{Hydrogen gas}}=663mmHg\times 0.388\\\\p_{\text{Hydrogen gas}}=257.24mmHg$

Hence, the partial pressure of nitrogen gas is 405.76 mmHg and that of hydrogen gas is 257.24 mmHg

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Answer:

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Explanation:

group can be taken from the electronic configuration here it is 2s2 2p2 so it should belongs to 4A or 14

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