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Shaking up a soda bottles increase pressure by adding the number of gas particles (moles of carbon dioxide) into the inflexible can. If a soda bottle has an initial pressure of 2.50 atm and 0.150mol of CO2, then is shaken up so there are now 0.500 moles of carbon dioxide, what will the new pressure of the soda bottle be?

Respuesta :

Answer : The new pressure of the soda bottle will be, 8.33 atm

Explanation :

As we know that:

PV=nRT

At constant volume and temperature of gas, the pressure will be directly proportional to the number of moles of gas.

The relation between pressure and number of moles of gas will be:

[tex]\frac{P_1}{P_2}=\frac{n_1}{n_2}[/tex]

where,

[tex]P_1[/tex] = initial pressure of gas = 2.50 atm

[tex]P_2[/tex] = final pressure of gas = ?

[tex]n_1[/tex] = initial number of moles of gas = 0.150 moles

[tex]n_2[/tex] = final number of moles of gas = 0.500 mol

Now put all the given values in the above expression, we get:

[tex]\frac{2.50atm}{P_2}=\frac{0.150mol}{0.500mol}[/tex]

[tex]P_2=8.33atm[/tex]

Therefore, the new pressure of the soda bottle will be, 8.33 atm

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