Final answer:
The pair of balloons that will deflate at the same rate are those containing ethene (C2H4) and nitrogen (N2) gases because they have the same molar mass, meaning they diffuse at equivalent rates according to Graham's Law of Effusion.
Step-by-step explanation:
The question pertains to the diffusion rates of gases from balloons based on the Graham's Law of Effusion, which states that the rate of effusion (or diffusion) of a gas is inversely proportional to the square root of its molar mass (molecular weight). Since all the balloons are at the same temperature and pressure, Avogadro's law applies, indicating that equal volumes of gases contain the same number of molecules. To find out which pair of balloons will deflate at the same rate, we need to compare the molar masses of the gases involved.
Calculating the molar mass of each gas: NH₃ (Ammonia) is 14 (N) + 1x3 (H) = 17 g/mol, CO₂ (Carbon Dioxide) is 12 (C) + 16x2 (O) = 44 g/mol, C₂H₄ (Ethene) is 12x2 (C) + 1x4 (H) = 28 g/mol, and N₂ (Nitrogen) is 14x2 (N) = 28 g/mol. Ethene (C₂H₄) and Nitrogen (N₂) both have the same molar mass of 28 g/mol, indicating they would effuse or diffuse at the same rate from their balloons..