It is not safe to put aerosol canisters in a campfire, because the pressure inside the canisters gets very high and they can explode. If you have a 1.0 liter canister that holds 2 moles of gas, and the campfire temperature is $$1400^\circ \mathrm{C}$$, what is the pressure inside the canister? (Use $$R = 0.0821\ \mathrm{L\ atm/(mol\ K)})$$

Q: It is not safe to put aerosol canisters in a campfire, because the pressure inside the canisters gets very high and they can explode. If you have a 1.0 liter canister that holds 2 moles of gas, and the campfire temperature is $$1400^\circ \mathrm{C}$$, what is the pressure inside the canister? (Use $$R = 0.0821\ \mathrm{L\ atm/(mol\ K)})$$

$$P = \frac{nRT}{V} = \frac{2 \times 0.0821 \times (1400 + 273)}{1.0} = 274.6\ \mathrm{atm}$$

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$$P = \frac{nRT}{V} = \frac{2 	imes 0.0821 	imes (1400 + 273)}{1.0} = 274.6\ \mathrm{atm}$$

Applying the Ideal Gas Law to Calculate Pressure in a Heated Canister

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