A sealed container has 1 mole of helium and 2 moles of nitrogen at 30DC when the total pressure of mixture is 0.60 atm what is the partial pressure of the nitrogen?

Answers

Answer 1
Answer:

Answer:

The partial pressure of  nitrogen is  0.402 atm.

Explanation:

Given data:

Number of moles of helium = 1 mol

Number of moles of nitrogen = 2 mol

Total pressure of mixture = 0.60 atm

Partial pressure of nitrogen = ?

Solution:

First of all we will calculate the mole fraction of nitrogen.

mole fraction of nitrogen = moles of nitrogen / total number of moles

mole fraction of nitrogen = 2 mol / 3 mol = 0.67

Partial pressure of nitrogen:

P₁ = [ n₁ /n(t)] × Pt

P₁ = 0.67 × 0.60 atm

P₁ = 0.402 atm

Answer 2
Answer:

Final answer:

To find the partial pressure of nitrogen in a mixture, calculate the mole fraction of nitrogen and multiply it by the total pressure of the mixture. In this case, the partial pressure of nitrogen is 0.40 atm.

Explanation:

The question is about determining the partial pressure of nitrogen in a mixture of helium and nitrogen based on Dalton's Law of Partial Pressures. First, we find the mole fraction of nitrogen, which is the ratio of moles of nitrogen to the total moles in the mixture. In this scenario, the mole fraction (XN2) is 2 moles of nitrogen divided by the total moles (1 mole of helium + 2 moles of nitrogen), which equals 2/3.

Then we use Dalton's Law, which states that the partial pressure of nitrogen (PN2) can be found by multiplying the mole fraction by the total pressure of the mixture. Therefore, the partial pressure of nitrogen is 0.60 atm (total pressure) multiplied by 2/3 (mole fraction of nitrogen), yielding a partial pressure for nitrogen of 0.40 atm.

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Answers

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Answers

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Answers

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Answers

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Answers

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Under which color of light will plants be least likely to make food?
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Answers

Answer:

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Explanation:

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Other options:

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Answer:

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Explanation: