Question
Asked Feb 22, 2020
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A 15.0-L tank is filled with helium gas at a pressure of
1.00 x 102 atm. How many balloons (each 2.00 L) can be
inflated to a pressure of 1.00 atm, assuming that the temperature
remains constant and that the tank cannot be
emptied below 1.00 atm?

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Expert Answer

Given data:

Chemistry homework question answer, step 1, image 1

Calcuklations:

The number of moles of helium is calculated by the formula shown below.

Chemistry homework question answer, step 2, image 1

Substitute the volume as 15.0 L and pressure as 1.00 × 102 atm in equation (I) to calculate the number of moles of helium gas in the tank.

Chemistry homework question answer, step 2, image 2

It was given that tank cannot be emptied below 1.0 atm. Therefore, the number of moles of helium that is remain in the tank is calculated as shown below.

Chemistry homework question answer, step 2, image 3

Therefore, the number of moles of helium gas transferred from the tank to balloons is calculated as shown below.

Chemistry homework question answer, step 2, image 4

Substitute the volume as 2.0 L and pressure as 1.00 atm in equation (I) to calculate the number of moles of helium gas in each balloon.

Chemistry homework question answer, step 2, image 5

The number of balloons is calculated as shown below.

Chemistry homework question answer, step 2, image 6

Since the number of balloons can not be in fraction or in decimal. Therefore, the number of balloons will be 742.

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