33. If \( 140 \mathrm{~cm}^{3} \) of methane diffuse into air in 72 seconds hew leng will it take \( 210 \mathrm{~cm}^{3} \) of susphut dioride to diffuse inder the same conditions? 34. The temprature of \( 2 s ~ L \) of a qas inctially at sip is raised to \( 250^{\circ} \mathrm{C} \) at constant volisme: calculate the final pressure. of the gas is atmosphere.

When we consider the diffusion of gases, we can refer to Graham's Law, which states that the rate of diffusion of a gas is inversely proportional to the square root of its molar mass. Since methane (CH₄) has a molar mass of about 16 g/mol and sulfur dioxide (SO₂) has a molar mass of approximately 64 g/mol, we can deduce that sulfur dioxide will diffuse slower. Thus, if methane diffuses 140 cm³ in 72 seconds, 210 cm³ of sulfur dioxide would take about 288 seconds to diffuse under identical conditions. To find the final pressure of a gas when its temperature changes, we can use the Ideal Gas Law and the concept of absolute temperature. First, convert \( 250^\circ C \) to Kelvin by adding 273.15, giving us 523.15 K. Using the ratio of the temperatures and initial conditions, the final pressure \( P_2 \) can be found using the equation \( P_2 = P_1 \times \frac{T_2}{T_1} \). If we assume the initial pressure \( P_1 \) is 1 atm at 293.15 K (20°C), then \( P_2 \) would be approximately 1.78 atm when the gas is heated to 523.15 K.