Question

In a container, 1 g of hydrogen and 1 g of oxygen are taken. Find the ratio of hydrogen pressure to oxygen pressure.

Answer 1

Step 1: Apply the ideal gas law.

For an ideal gas: \[ P = \frac{nRT}{V} \] Given that \( R, T, V \) are constant for both gases, the pressure ratio is equivalent to the mole ratio: \[ \frac{P_H}{P_O} = \frac{n_H}{n_O} \]

Step 2: Determine the moles of each gas.

Moles of hydrogen (\( H_2 \)): \[ n_H = \frac{\text{mass}}{\text{molar mass}} = \frac{1}{2} = 0.5 \]

Moles of oxygen (\( O_2 \)): \[ n_O = \frac{1}{32} = 0.03125 \]

Step 3: Calculate the pressure ratio.

\[ \frac{P_H}{P_O} = \frac{n_H}{n_O} = \frac{0.5}{0.03125} = 16 \]

Final Answer:

\[ \boxed{\frac{P_H}{P_O} = 16} \]