4. Use the pressure of the butane gas (1.1705), along with the temperature and volume recorded in the lab, to determine the moles of butane gas collected in the lab. You will use the ideal gas law (and the ideal gas constant, R) for this calculation; just make sure that all of the measurements have the correct units necessary for the calculation.

Data Table
mass of lighter before (g) 32.105 g
volume of butane gas collected (mL) 90. mL
mass of Lighter after (g) 31.844 g
room temperature (K) 297 K
air pressure (atm) 1.2 atm

Temperature (°C) Pressure of Water Vapor (atm)
20.0 0

Question

4.	Use the pressure of the butane gas (1.1705), along with the temperature and volume recorded in the lab, to determine the moles of butane gas collected in the lab. You will use the ideal gas law (and the ideal gas constant, R) for this calculation; just make sure that all of the measurements have the correct units necessary for the calculation.



Data Table 
mass of lighter before (g)	32.105 g
volume of butane gas collected (mL)	90. mL
mass of Lighter after (g)	31.844 g
room temperature (K)	297 K
air pressure (atm)	1.2 atm


Temperature (°C)	Pressure of Water Vapor (atm)
20.0	0

jfraser · Answer

What does the ideal gas law say about moles (and pressure, volume, and temperature)?