The air in a bicycle tire is bubbled through water and collected at&nbsp;25∘C. If the total volume of gas collected is 5.45 L at a temperature of&nbsp;25∘C&nbsp;and a pressure of 745 torr, how many moles of gas were in the bicycle tire?

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The air in a bicycle tire is bubbled through water and collected at&amp;nbsp;25∘C. If the total volume of gas collected is 5.45 L at a temperature of&amp;nbsp;25∘C&amp;nbsp;and a pressure of 745 torr, how many moles of gas were in the bicycle tire?

Froldigh · Accepted Answer

Step 1T=(25+273.15)K=298.15KP→t=745→rr=745mmHgPH2O=23.78mmHgV=5.45Lngas=?Write down the known and unknown values.Step 2P→t=PH2O+PgasPgas=P→t−PH2O=745mmHg−−23.7mmHg=721.3mmHgTo determine the evolved gas&#039;s partial pressure, use the gas-evolution equation based on Dalton&#039;s Law of&amp;nbsp;Step 3Pgas=721.3m̸m̸H̸g1atm&amp;nbsp;760m̸m̸H̸g=0.94908atmConvert the evolved gas&#039;s partial pressure into atmospheres.Step 4PgasV=ngasRT&amp;nbsp;ngas=PgasVRT&amp;nbsp;=0.94908a̸t̸m̸mol⋅K̸5.45L̸&amp;nbsp;0.08206L̸⋅a̸t̸m̸298.15K̸=0.211molTo determine how many moles of the evolved gas there are, use the Ideal Gas Law.

Jazz Frenia · Accepted Answer

To solve this problem, we can use the ideal gas law equation:PV=nRTWhere:- P is the pressure of the gas (in atm)- V is the volume of the gas (in liters)- n is the number of moles of gas- R is the ideal gas constant (0.0821 L·atm/mol·K)- T is the temperature of the gas (in Kelvin)First, let&#039;s convert the given pressure from torr to atm. We know that 1 atm is equal to 760 torr. Therefore:P=745torr760torr/atm=0.979atmNext, let&#039;s convert the given volume to liters:V=5.45LNow, we can rearrange the ideal gas law equation to solve for the number of moles:n=PVRTSubstituting the given values:n=(0.979atm)(5.45L)(0.0821L·atm/mol·K)(25+273.15)Kn=5.34L·atm22.42L·atm/mol·Kn=0.237molHowever, we need to account for the fact that the gas was collected at 25 degrees Celsius, not Kelvin. To convert the temperature from Celsius to Kelvin, we add 273.15:n=0.237mol×298.15K273.15Kn=0.260molTherefore, the number of moles of gas in the bicycle tire is approximately 0.260 mol, rounded to three decimal places.

Andre BalkonE · Accepted Answer

Given:Total volume of gas collected, V=5.45LTemperature, T=25°CPressure, P=745torrTo find the number of moles of gas, we can use the ideal gas law equation:PV=nRTFirst, we need to convert the temperature from Celsius to Kelvin. We use the equation:T(K)=T(°C)+273.15Plugging in the given values:T=25°C+273.15=298.15KNow, we can rearrange the ideal gas law equation to solve for the number of moles:n=PVRTSubstituting the given values:n=(745torr)(5.45L)(0.0821L&amp;nbsp;atm/(mol&amp;nbsp;K))(298.15K)Simplifying the equation gives us:n=0.211molTherefore, there were 0.211 moles of gas in the bicycle tire.Hence, the solution to the problem is 0.211 mol.

Mr Solver · Accepted Answer

First, we need to convert the temperature from Celsius to Kelvin using the equation:T(K)=T(°C)+273.15Plugging in the values, we get:T(K)=25+273.15=298.15Now we can rearrange the ideal gas law equation to solve for n:n=PVRTPlugging in the values, we get:n=(745torr)×(5.45L)(0.0821L·atm/(mol·K))×(298.15K)Simplifying the equation, we find:n=4061.7524.457mol≈166.26molTherefore, there were approximately 166.26 moles of gas in the bicycle tire.(Note: We should round the final answer to the appropriate number of significant figures based on the given data. In this case, since the total volume of gas collected is given with three significant figures, the final answer should be rounded to three significant figures as well.)

The air in a bicycle tire is bubbled through water and collected at 25^{\circ

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