Question

question 20 4 pts there are two samples of gas in 10l containers at standard temperature; one contains 1.0 mole of methane, ch₄,the other 1.0 mole of molecular nitrogen, n₂. which container has a higher pressure? the methane container the nitrogen container neither container

Explanation:

Step1: Recall Ideal Gas Law

The ideal gas law is \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is moles, \( R \) is gas constant, and \( T \) is temperature.

Step2: Analyze Given Conditions

Both gases are in 10L containers (\( V \) same), at standard temperature (\( T \) same), and have 1.0 mole (\( n \) same). \( R \) is a constant.

Step3: Compare Pressures

From \( PV = nRT \), rearranged to \( P=\frac{nRT}{V} \). Since \( n \), \( R \), \( T \), and \( V \) are identical for both, \( P \) must be equal for both methane and nitrogen.

Answer:

Neither Container