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AysviL [449]
3 years ago
5

When pumping air into a tire, you have to pull back on the pump plunger to fill the pump with air. This increases the volume of

the air inside the pump. This increase in volume has what effect on the gases inside the pump?
Question 9 options:

the gas molecules inside the pump are able to spread out more which decreases the pressure of the gas.


the gas molecules inside the pump get compressed and packed closer together which decreases the pressure of the gas.


the gas molecules inside the pump are able to spread out more which increases the pressure of the gas.


the gas molecules inside the pump get compressed and packed closer together which increases the pressure of the gas.
Chemistry
2 answers:
Monica [59]3 years ago
5 0
6969696969 there hope
Levart [38]3 years ago
4 0

Answer:

Pulling back on the plunger allows you to put in more air into the pump and the more air you have inside a fixed volume, the greater the pressure becomes. (D)

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Determine the partial pressure and number of moles of each gas in a 15.75-L vessel at 30.0 C containing a mixture of xenon and n
lawyer [7]

Answer:

The Partial pressure of Xe and Ne will be 4.95 atm and 1.55 atm. The number of moles of Xe and Ne will be 3.13 and 0.981

Explanation:

Let the total pressure of the vessel= 6.5 atm and mole fraction of Xenon= 0.761

As we know,

\chi_{Ne} + \chi_{Xe} = 1\\\chi_{Ne}= 1- 0.761\\\chi_{Ne}= 0.239

According to Dalton's Law of partial pressure-

P_i=\chi_i\times P_{total}

Where,

P_i=The pressure of the gas component in the mixture

\chi_i= Mole fraction of that gas component

P_t= The total pressure of the mixture

P_{Xe}=(0.761)\times(6.5)\\P_{Xe}= 4.95 atm\\\\\\P_{Ne}=(0.239)\imes (6.5)\\P_{Ne}= 1.55 atm

<u>Calculation: </u>

To calculate the number of moles,

PV=nRT

n=\frac{PV}{RT}

n_{Xe}= \frac{4.95\times 15.75}{0.0821\times303 }\\ n_{Xe}= \frac{77.96}{24.87} \\n_{Xe}= 3.13\,mole \\\\\\n_{Ne}= \frac{1.55\times 15.75}{0.0821\times303 }\\\\n_{Ne}=\frac{24.41}{24.87}\\ n_{Ne}=0.981 \,mole

Learn more about Dalton's Law of partial pressure here;

brainly.com/question/14119417

#SPJ4

4 0
1 year ago
Can you help me understand this ? I completely dont understand it ​. i know the tire will burst.
icang [17]

Answer:

There is only one formula to use and we should assume ideal gas. This equation is: PV=nRT. For the following questions manipulate this equation to get the answer.

1. n = PV/RT = (249*1000 Pa)(15.6 L)(1 m^3/1000 L)/(8.314 Pa-m^3/mol-K))(21+273) = 1.59 mol

2. P = nRT/V = (1.59)(8.314)(51+273)/(15.6/1000)(1000) = 274.55 kPa

3. Since the answer in #2 is more than 269 kPa, then the tires will likely burst. 4. Reduce pressure way below the limit 269 kPa.

Explanation:

6 0
3 years ago
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