The gas pressure in an aerosol can is 1.8 atm at 25^$\circ$C. If the gas is an ideal gas, what pressure would develop in the can if it were heated to 475^$\circ$C A) 0.095 atm B) 0.72 atm C) 3.3 atm D) 4.5 atm E) 34 atm

Question

Quizplus · Accepted Answer

We can use the ideal gas law equation:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

We can assume that the number of moles and the volume of the gas remain constant, since the can is sealed. Therefore, we can write:

P₁/T₁ = P₂/T₂

where P₁ is the initial pressure (1.8 atm), T₁ is the initial temperature in Kelvin (25+273=298 K), P₂ is the final pressure (unknown), and T₂ is the final temperature in Kelvin (475+273=748 K).

Solving for P₂, we get:

P₂ = P₁(T₂/T₁) = 1.8(748/298) = 4.5 atm

Therefore, the answer is D.

The Gas Pressure in an Aerosol Can Is 1 ∘\circ∘ C If the Gas Is an Ideal Gas, What Pressure

The Gas Pressure in an Aerosol Can Is 1 $\circ$ C If the Gas Is an Ideal Gas, What Pressure