Question

determine the temperature of 2.49 grams of carbon dioxide gas that is in a 565.0 ml container at a pressure of 143 kpa. which gas law equation should be used to solve this problem? pv = nrt p₁v₁ = p₂v₂ v₁/n₁ = v₂/n₂ p₁/t₁ = p₂/t₂ v₁/t₁ = v₂/t₂ p₁v₁/t₁ = p₂v₂/t₂

Explanation:

The ideal gas law \(PV = nRT\) is used when we have pressure (\(P\)), volume (\(V\)), amount of substance (\(n\)), and temperature (\(T\)) related. Here, we have pressure (\(P = 143\ kPa\)), volume (\(V=565.0\ mL\)), mass of \(CO_2\) (from which we can find \(n\) using molar mass), and we need to find \(T\). The other equations: \(P_1V_1 = P_2V_2\) (Boyle's law, for constant \(n\) and \(T\)), \(\frac{V_1}{n_1}=\frac{V_2}{n_2}\) (Avogadro's law, for constant \(P\) and \(T\)), \(\frac{P_1}{T_1}=\frac{P_2}{T_2}\) (Gay - Lussac's law, for constant \(V\) and \(n\)), \(\frac{V_1}{T_1}=\frac{V_2}{T_2}\) (Charles's law, for constant \(P\) and \(n\)), \(\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}\) (combined gas law, for same amount of gas \(n\)) are not applicable as they assume some variables constant which is not the case here. We need an equation that relates all \(P\), \(V\), \(n\), \(T\) without assuming constancy of \(n\) (since we calculate \(n\) from mass) and other variables.

Answer:

\(PV = nRT\)