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Anna [14]
3 years ago
11

A mixture of He, Ne, and N2 gases has a pressure of 0,898 atm. If the pressures of He and Ne are 0.336 atm and 0.106 atm, respec

tively, what is the partial pressure of N2 in the mixture?
Chemistry
1 answer:
Alchen [17]3 years ago
5 0

Answer:

Pressure for N₂ = 0.456 atm

Explanation:

There is law for gases which states that the sum of partial pressures of each gas in a mixture, is equal to the total pressure of the system.

For this case, we have a mixture of He, Ne and N₂

Then Total pressure is 0.898 atm

He's pressure + Ne's pressure + N₂'s pressure = 0.898 atm

N₂'s pressure = 0.898 atm - 0.336 atm - 0.106 atm

Pressure for N₂ = 0.456 atm

This is called the Dalton's law of partial pressures.

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Explain why copper is used for the<br> roofs of some buildings and magnesium is not.
Scrat [10]

Answer:

Because of the less reactivity of copper.

Explanation:

As well as being resistant to the elements and thereby less likely to be affected by rainfall, hail, and mildew than other types of roofing, copper is also one of the most fireproof materials available. Copper is also highly resistant to thermal changes and thereby doesn't deteriorate quickly.

Magnesium would also corrode PDQ. Magnesium sheeting would also pose an unacceptably high fire hazard.

3 0
2 years ago
In the engineering design process what do engineers do immediately after testing a prototype
mote1985 [20]

Answer:

Iterate to improve the solution

Explanation:

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5 0
3 years ago
Which of the following is true regarding atomic radius?
Ymorist [56]

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5 0
3 years ago
A container of hydrogen gas has the same temperature as a container of oxygen gas. The gas atoms having the greater average kine
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Answer:

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4 0
2 years ago
What mass of CO was used up in the reaction with an excess of oxygen gas if 24.7g of carbon dioxide is formed? 2 CO + O2 &gt; 2
Zolol [24]
Balance Chemical Equation,
                                      2 CO  +  O₂   →   2CO₂
Acc. to this reaction,
88 g (2 mole) of CO₂ was produced when  =  56 g (2 mole)of CO was reacted
So, 
24.7 g of CO₂ will be produced by reacting =  X g of CO

Solving for X,
                                    X  =  (56 g × 24.7 g) ÷ 88 g

                                    X  =  2.26 g ÷ 88 g

                                    X  =  0.0257 g of CO

Result:           
            0.0257 g of CO is required to be reacted with excess of O₂ to produce 24.7 g of CO₂.
7 0
2 years ago
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