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kompoz [17]
3 years ago
11

a gas mixture is exerting a pressure of 1.04 atm inside a sealed container. The gas was found to be a mixture of carbon dioxide

and nitrogen gas. If the mixture is 42% CO2, what is the partial pressure of nitrogen
Chemistry
1 answer:
qwelly [4]3 years ago
5 0

Answer:

Partial pressure of Nitrogen = 0.6032 atm

Explanation:

According to Dalton's law of partial pressure, at constant temperature, the total pressure exerted by a mixture of gases that do not react with one another is a sum of the partial pressures of the individual gases. And the partial pressure of each gas is proportional to their percentage composition. The partial pressure of each as is given as

Partial Pressure = (Percentage composition) × (Total pressure)

In this question, a gas mixture of Carbon dioxide and Nitrogen exerts a total pressure of 1.04 atm

The mixture contains 42% CO₂, meaning it contains 100-42 = 58% of Nitrogen.

Partial Pressure of Nitrogen = 0.58 × 1.04 = 0.6032 atm

Hope this Helps!!!

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How many moles of nitrogen trifluoride (NF3) can be produced from 9.65 mole of Fluorine gas (F2)
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Answer:

6.43 moles of NF₃.

Explanation:

The balanced equation for the reaction is given below:

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From the balanced equation above,

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Finally, we shall determine the number of mole of nitrogen trifluoride (NF₃) produced by the reaction of 9.65 moles of Fluorine gas (F₂). This can be obtained as follow:

From the balanced equation above,

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Therefore, 9.65 moles of F₂ will react to to produce = (9.65 × 2)/3 = 6.43 moles of NF₃.

Thus, 6.43 moles of NF₃ were obtained from the reaction.

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