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tangare [24]
3 years ago
11

If a gas occupies 22.4 L at 0.265 atm, then what will the pressure be in atmospheres if the gas occupies 35.52 L? Assume all oth

er
variables are held constant
A)0.167 atm
B)0.437 atm
C)0.886 atm
D)149 atm
Chemistry
1 answer:
pochemuha3 years ago
8 0

Answer:

The new pressure is 0.167 atm

The correct answer is option A

Explanation:

Step 1: Data given

Volume of the gas = 22.4 L

Pressure of the gas = 0.265 atm

The volume increases to 35.52 L

Step 2: Calculate the new pressure

P1*V1 = P2*V2

⇒with P1 = the initial pressure = 0.265 atm

⇒with V1 = the initial volume = 22.4 L

⇒with P2 = the new pressure = TO BE DETERMINED

⇒with V2 = the increased volume = 35.52 L

0.265 atm * 22.4 L = P2 * 35.52 L

P2 = (0.265 atm * 22.4 L) / 35.52 L

P2 = 0.167 atm

The new pressure is 0.167 atm

The correct answer is option A

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A sample of gas has an initial pressure of 1.5 atm, an initial volume of 3.0 L, and an initial temperature of 293K. If the final
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1.9 L

Explanation:

Step 1: Given data

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  • Final pressure (P₂): 2.5 atm
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Step 2: Calculate the final volume of the gas

If we assume ideal behavior, we can calculate the final volume of the gas using the combined gas law.

P₁ × V₁ / T₁ = P₂ × V₂ / T₂

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V₂ = 1.5 atm × 3.0 L × 303 K / 293 K × 2.5 atm = 1.9 L

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Nitric acid, , is manufactured by the Ostwald process, in which nitrogen dioxide, , reacts with water. How many grams of nitroge
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Explanation:

Let's consider the reaction in the last step of the Ostwald process.

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The molar ratio of NO₂ to HNO₃ is 3:2. The reacting moles of NO₂ are:

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The molar mass of NO₂ is 46.01 g/mol. The mass corresponding to 0.153 moles is:

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