Ideal gas law is an equation of state that relates the pressure, volume and temperature for a given mass of an ideal gas.

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Consider the statement about the ideal gas law and what it relates.

Option 1 (True): The ideal gas law is PV = nRT, which indeed relates pressure (P), volume (V), and temperature (T) for a specified amount of gas, quantified by n (moles). If you are given a fixed mass of a specific gas, you can convert that mass to moles using the molar mass, so n is fixed for that scenario. Consequently, for that fixed amount, P, V, and T are related by PV = nRT. The phrase 'for a given mass' is effectively a way of fixing the amount of substance when the molar mass is known, so the equation applies.

Option 2 (False): If one were to interpret 'ideal gas law' as not applying to a fixed quantity of gas, or to deny the mass-to-moles relationship, it would be incorrect. The law fundamentally requires knowledge of the amount of substance; without fixing n (or mass and molar mass to determine n), the relationship among P, V, and T cannot be uniquely determined. This option neglects the essential role of n in the equation and would misrepresent the core purpose of the equation of state for an ideal gas.

Option 3 (False): Claiming that the law relates only two variables or excludes mass-related considerations would be misleading. The standard formulation explicitly includes n (or amount) to tie P, V, and T together for a given quantity of gas. Disregarding n ignores a fundamental aspect of the equation of state.

Option 4 (False): Suggesting that the law applies regardless of the amount of gas without specifying n would be incorrect. The relationship among P, V, and T is contingent on how much gas is present, as encapsulated by n; without that, the law does not uniquely connect the variables.

CLMTGR5001_002_2025_3 - Dynamics of Climate Variability and Chan Quiz 3b1 Week 3 Lecture 2.1 - OPTIONAL

Ideal gas law is an equation of state that relates the pressure, volume and temperature for a given mass of an ideal gas.

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