The air in a bicycle tire is bubbled through water and collected at ${25}^{\circ}C$. If the total volume of gas collected is 5.45 L at a temperature of ${25}^{\circ}C$ and a pressure of 745 torr, how many moles of gas were in the bicycle tire?

alka8q7
2021-11-17
Answered

The air in a bicycle tire is bubbled through water and collected at ${25}^{\circ}C$. If the total volume of gas collected is 5.45 L at a temperature of ${25}^{\circ}C$ and a pressure of 745 torr, how many moles of gas were in the bicycle tire?

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Froldigh

Answered 2021-11-18
Author has **17** answers

Step 1

Write down the known and unknown values.

Step 2

Use the gas-evolution equation based on Dalton's Law of partial pressures to calculate the partial pressure of the gas evolved.

Step 3

Convert the partial pressure of the evolved gas into atmospheres.

Step 4

Use the Ideal Gas Law to calculate the number of moles of the evolved gas.

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A healthcare provider monitors the number of CAT scans performed each month in each of its clinics. The most recent year of data for a particular clinics follows (the reported variable is the number of CAT scans each month expressed as the number of CAT scans per thousand members of the health plan):

2.31,2.09,2.36,1.95,1.98,2.25,2.16,2.07,1.88,1.94,1.97,2.02.

Find a two-sided

Round your answers to two decimal places (e.g. 98.76).