Question

which of the following variables is not correctly matched with its value for this problem: what pressure is required to contain 0.023 moles of nitrogen gas in a 4.2 l container at a temperature of 20°c? r = 0.0821 l·atm/mol·k p = 20°c v = 4.2 l n = 0.023 mol

Explanation:

Step1: Convert temperature to Kelvin

The ideal gas law uses temperature in Kelvin. The conversion formula is \( T(K)=T(^{\circ}C)+273.15 \). Given \( T = 20^{\circ}C \), then \( T=(20 + 273.15)K=293.15K \). But the value \( P = 20^{\circ}C \) is wrong because \( P \) represents pressure, and the unit \( ^{\circ}C \) is for temperature.

Answer:

The variable \( P = 20^{\circ}C \) is not correctly matched. Pressure (\( P \)) should have units like atm, Pa, etc., not \( ^{\circ}C \) (which is for temperature).