Answer:
Higher pressure, is the right answer.
Explanation:
The A will have a higher pressure. Since we have given the volume and temperature is same in both containers A and B. Below is the calculation for proof that shows which container has the higher pressure while keeping the volume and temperature the same.
[tex]So, \ V_A = V_B \\\frac{n_A T_A}{P_A} = \frac{n_B T_B}{P_B} \\Here, \ T_A = T_B \\P_A = \frac{n_A}{n_B} \times P_B \\\frac{n_A}{n_B} > 1 \\\frac{P_A}{P_B} > 1 \\P_A > P_B \\[/tex]
Therefore, the container “A” will have higher pressure.
Container A will have a higher pressure than container B.
According to the approximations of ideal gas conditions, the pressure of a gas is directly proportional to the number of molecules of a gas at constant temperature and volume.
Having this in mind, at constant temperature and volume, container A has more gaseous molecules than B, then container A will have a higher pressure than container B.
Missing parts;
If two separate containers A and B have the same volume and temperature, but container A has more gaseous molecules than B, then container A will have: A) Higher pressure B) Lower pressure C) A greater universal gas constant D) A smaller universal gas constant
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