Q1. If I have a 1.0 liter canister that holds 2 moles of gas, and the campfire temperature is 1400°C, what is the pressure inside the canister?

Background

Topic: Ideal Gas Law

This question tests your ability to use the ideal gas law to predict the pressure inside a container when the temperature is extremely high. It also highlights the safety risks associated with heating pressurized containers.

Key formula:

Where:

• = pressure (in atm)

• = volume (in liters)

• = number of moles (here, 2 moles)

• = ideal gas constant ( L·atm/mol·K)

• = temperature in Kelvin (must convert from Celsius)

Step-by-Step Guidance

1. Identify the known values: L, mol, C.

2. Convert the temperature from Celsius to Kelvin: K.

3. Write the ideal gas law formula and rearrange to solve for pressure: .

4. Check that all units are compatible with the gas constant (L, atm, mol, K).

5. Set up the calculation by plugging in the values: .

Try solving on your own before revealing the answer!