The air in a bicycle tire is bubbled through water and collected at 25 C. If the total volume of gas collected is 5.65 L at a temperature of 25 C and a pressure of 749 torr how many moles of gas w?

To find the number of moles of gas collected, we can use the ideal gas law, ( PV = nRT ), where ( P ) is the pressure in atmospheres, ( V ) is the volume in liters, ( n ) is the number of moles, ( R ) is the ideal gas constant (0.0821 L·atm/(K·mol)), and ( T ) is the temperature in Kelvin. First, convert the pressure from torr to atm (749 torr ÷ 760 torr/atm = 0.983 atm) and the temperature to Kelvin (25 C + 273.15 = 298.15 K).

Now, rearranging the ideal gas law to solve for ( n ):
[ n = \frac{PV}{RT} = \frac{(0.983 , \text{atm})(5.65 , \text{L})}{(0.0821 , \text{L·atm/(K·mol)})(298.15 , \text{K})} \approx 0.23 , \text{moles} ]