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3 years ago

Using the van der Waals equation, determine the pressure exerted by 4.30 mol Ar in 3.6 L at 325K.

Chemistry

1 answer:

Vika [28.1K]3 years ago

5 0

Answer:

37.7 atm

Explanation:

Using the relation;

(P + an^2/V^2) (V - nb) = nRT

(P + an^2/V^2) = nRT/(V - nb)

a = 0.0341 atm dm^2 Mol^2

b = 0.0237 dm/mol

P = nRT/(V - nb) - an^2/V^2

P = [4.3 * 0.082 * 325 / (3.6 - (4.3 * 0.0237))] - (0.0341 * (4.3^2))/(3.6^2)

P = 114.595/(3.498) - 0.0487

P = 37.7 atm

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IceJOKER [234]

Concepts used:

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003 - Number of CaH₂ formula units in 6.065 grams

Number of Moles:

We know that the molar mass of CaH₂ is 42 grams/mol

Number of Moles of CaH₂ = given mass/molar mass

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Number of formula units = number of moles * 6.022*10²³

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Number of Moles:

We mentioned this formula before:

Number of formula units = number of moles * 6.022*10²³

Solving it for number of moles, we get:

Number of moles = Number of Formula units / 6.022* 10²³

replacing the variable

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Number of moles= 10.5 moles

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005 - Number of moles in 9.78 * 10²¹ formula units of CeI₃

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We have the formula:

Number of moles = Number of Formula units / 6.022* 10²³

replacing the variables

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2 years ago

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3 years ago

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Andre45 [30]

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natima [27]

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2 years ago

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Dmitrij [34]

Answer:

<h2>127.57 moles</h2>

Explanation:

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From the question we have

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We have the final answer as

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Hope this helps you

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2 years ago