Does butane follow the ideal gas law?
Although butane can be described by the ideal gas law, it is important to remember that it is not ideal. With the volume, temperature, and pressure of butane, you can use the ideal gas law to find the moles of butane released from the lighter.
Why is butane not an ideal gas?
Under a moderate amount of pressure, the butane (iso-butane actually) is in the liquid state at room temperature. We know that the pressure can’t be too high, because the lighter is made of fairly thin plastic that would not stand a high pressure.
Which gas law should be used in order to determine the pressure of the dry butane in the graduated cylinder?
The ideal gas law
The ideal gas law relates the four measurable properties of a gas, (P, V, n, T). In this experiment, the ideal gas law will be used to determine the molar mass of butane gas.
Why is the insolubility of butane in water critical to performing this experiment?
Possible answer: Butane is extremely flammable and will ignite. Possible answer: Because the butane will not dissolve in the water, it is possible for butane gas possible to form under water and get trapped.
How many moles does butane have?
Experimental molar mass (g/mole) of butane: 0.23 g/0.0040 moles = 58 g/mole 13. The molecular formula of butane is C4H10. Calculate its molar mass.
Why is the ideal gas law inaccurate?
Q: Why is the ideal gas law inaccurate? The ideal gas law is inaccurate because the ideal gas law accounts for no or negligible molecular interaction, while the real gases do have molecular interaction under certain conditions.
Is the ideal gas law valid for every gas?
Since ideal gas is defined as one in which all collisions between atoms or molecules are perfectly elastic. There are no intermolecular attractive forces, and there is no such thing in nature as a truly ideal gas. On the other hand, all real gases approach the ideal state at low pressures (densities).
What is the pressure of butane gas?
170 kPa
Butane
| Names | |
|---|---|
| Boiling point | −1 to 1 °C; 30 to 34 °F; 272 to 274 K |
| Solubility in water | 61 mg/L (at 20 °C (68 °F)) |
| log P | 2.745 |
| Vapor pressure | ~170 kPa at 283 K |
Which gas law should be used in order to determine the moles of butane used?
Use Avogadro’s law to determine the number of moles of butane gas. Assume that butane is an ideal gas and that one mole has a volume of 22.4 L at STP.