System 1 is 3.1 moles of a monatomic ideal gas held at a constant volume of 2.70 L as it undergoes a temperature increase.System 2 is 3.1 moles of a diatomic ideal gas held at a constant volume of 2.7 L as it undergoes a temperature increase equal to the temperature increase of System 1.The pressure increase for system 1 is ΔP₁ and for System 2 is ΔP₂ during the temperature increases.What is the ratio of ΔP₁/ΔP₂? A)1.0 B)0.60 C)1.7 D)2.5 E)4.5

Question

Quizplus · Accepted Answer

The pressure increase in an ideal gas due to temperature increase is given by the ideal gas law, $PV = nRT$, where $P$ is pressure, $V$ is volume, $n$ is the number of moles, $R$ is the ideal gas constant, and $T$ is temperature. For a constant volume process, the pressure increase is directly proportional to the temperature increase and the amount of substance (moles). Since both systems have the same number of moles and undergo the same temperature increase, the ratio of their pressure increases is 1.0, regardless of the gas being monatomic or diatomic. The heat capacity or specific heat does not affect the pressure increase directly in this scenario.

System 1 Is 3