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 735 torr, how many moles of gas was in the bicycle tire?
PV=nRT
solve for n. Use temp in kelvins.
R depends on units, I would shift to kpa, so make certain you use the right R.
0.21
To determine the number of moles of gas in the bicycle tire, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
We are given the following information:
Pressure (P) = 735 torr
Volume (V) = 5.65 L
Temperature (T) = 25°C = 298 K
The ideal gas constant (R) is typically expressed in units of atm·L/mol·K. Since the given pressure is in torr, we need to convert it to atm for consistency. There are 760 torr in 1 atm.
Step 1: Convert the pressure from torr to atm:
735 torr ÷ 760 torr/atm ≈ 0.966 atm
Now, we can rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT
Step 2: Plug in the values into the equation:
n = (0.966 atm) × (5.65 L) / [(0.0821 atm·L/mol·K) × 298 K]
Step 3: Calculate the number of moles:
n ≈ 0.23 moles
Therefore, there are approximately 0.23 moles of gas in the bicycle tire.