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erastova [34]
3 years ago
5

7. What is the total pressure of the following mixture of gases in a 20.0 L container at 298 K: 12.0 g He,

Chemistry
1 answer:
zloy xaker [14]3 years ago
5 0

Answer:

P(total) = 14.81 atm

Explanation:

According to the Dalton law of partial pressure,

The pressure exerted by mixture of gases are equal to the sum of partial pressure of individual gases.

P(total) = P1 + P2 + P3+ .....+ Pn

Given data:

Volume of container = 20.0 L

Temperature = 298 K

Mass of He = 12.0 g

Moles of hydrogen = 4.00 mol

Pressure of Ne = 6.25 atm

Solution:

Moles of helium:

Number of moles = mass/molar mass

Number of moles = 12 g/ 4 g/mol

Number of moles = 3 mol

Pressure of helium:

PV = nRT

P = nRT/ V

P = 3 mol × 0.0821 atm.L. mol⁻¹.k⁻¹ × 298 K / 20 L

P = 73.4 atm / 20

p = 3.67 atm

Pressure of hydrogen:

PV = nRT

P = nRT/ V

P = 4 mol × 0.0821 atm.L. mol⁻¹.k⁻¹ × 298 K / 20 L

P = 97.86 atm / 20

P = 4.89 atm

Total pressure:

P(total) = P(He) + P(Ne) + P(H₂)

P(total) = 3.67 atm + 6.25 atm + 4.89 atm

P(total) = 14.81 atm

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Answer:

Option (d) is correct

N³⁻ > F⁻ > Mg²⁺ > Si⁴⁺

Explanation:

Total electrons for all the species = 10

So these are <u>iso electronic</u> with each other.

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Ionic radii ∝ \frac{Magnitude of Negative Charge}{Magnitude of Positive Charge}

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One of the intermediates in the synthesis of glycine from ammonia, carbon dioxide, and methane is aminoacetonitrile, C2H4N2. The
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Answer:

Mass of C₂H₄N₂ produced = 3.64 g

Explanation:

The balanced chemical equation for the reaction is given below:

3CH₄ (g) + 5CO₂ (g) + 8NH₃ (g) → 4C₂H₄N₂ (g) + 10H₂O (g)

From the equation, 3 moles of CH₄ reacts with 5 moles of CO₂ and 8 moles of NH₃ to produce 4 moles of C₂H₄N₂ and 10 moles of H₂O

Molar masses of the compounds are given below below:

CH₄ = 16 g/mol; CO₂ = 44 g/mol; NH3 = 17 g/mol; C₂H₄N₂ = 56 g/mol; H₂O g/mol

Comparing the mole ratios of the reacting masses;

CH₄ = 1.65/16 = 0.103

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converting to whole number ratios by dividing with the smallest ratio

CH₄ = 0.103/0.103 = 1

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Multiplying through with 5

CH₄ = 1 × 5 = 5

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8 × 17 g (136 g) of NH₃ reacts to produce 4 × 56 g (224 g) of C₂H₄N₂

Therefore, 2.21 g of NH₃ will produce (2.21 × 224)/136 g of C₂H₄N₂ = 3.64 g of C₂H₄N₂

Mass of C₂H₄N₂ produced = 3.64 g

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