Question

the diagrams below show two pure samples of gas in identical closed, rigid containers. gas b has a higher temperature than gas a. there are also more particles in gas b than in gas a. which has the higher gas pressure? gas a gas b neither; their gas pressures are the same

Explanation:

Step1: Recall the ideal gas law

The ideal gas law is \(PV = nRT\). Here, \(P\) is pressure, \(V\) is volume (containers are identical, so \(V\) is the same for both gases), \(n\) is the number of moles (more particles in gas B means \(n_B>n_A\)), \(R\) is the gas constant, and \(T\) is temperature (\(T_B > T_A\)).

Step2: Analyze the effect of \(n\) and \(T\) on \(P\)

Since \(V\) and \(R\) are constant, \(P\propto nT\). Gas B has a higher \(n\) (more particles) and a higher \(T\) (higher temperature) compared to gas A. So, \(n_BT_B>n_AT_A\).

Answer:

gas B