Question

the diagrams to the right show the distribution and arrangement of gas particles in two different containers. according to kinetic - molecular theory, which of the following statements is true? check all that apply. if the temperatures of both containers are equal, container a has greater pressure than container b. if the volume of container a decreased, its pressure would decrease. if the pressure in both containers is equal, container a has a lower temperature than container b. done

Explanation:

• For the first statement: According to the ideal gas law \(PV = nRT\), when \(T\) (temperature) and \(V\) (volume) are constant, \(P\propto n\) (pressure is proportional to the number of moles). If temperatures are equal and assuming same - volume (from the diagrams, container A has more gas particles, so \(n_A>n_B\)). By \(P=\frac{nRT}{V}\), \(P_A > P_B\) when \(T\) and \(V\) are the same.
• For the second statement: Using \(P=\frac{nRT}{V}\), when \(n\) (number of moles), \(R\) (gas constant) and \(T\) (temperature) are constant, \(P\propto\frac{1}{V}\). If \(V\) decreases, \(P\) increases, not decreases.
• For the third statement: From \(P=\frac{nRT}{V}\), when \(P\) is constant, \(T=\frac{PV}{nR}\). Container A has more particles (\(n_A>n_B\)) and assuming same - pressure. If \(P\) is the same, \(T_A=\frac{P V}{n_A R}\) and \(T_B=\frac{P V}{n_B R}\). Since \(n_A > n_B\), \(T_A

Answer:

• If the temperatures of both containers are equal, container A has greater pressure than container B.
• If the pressure in both containers is equal, container A has a lower temperature than container B.