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

The correct answer is 16.

To find the ratio of hydrogen pressure to oxygen pressure, we use the ideal gas law:
$PV=nRT$

In this system, both gases are in the same container. Therefore, they share the same volume ($V$) and temperature ($T$). The gas constant ($R$) is also constant. Thus, the pressure ($P$) of each gas is directly proportional to the number of moles ($n$) of that gas:
$P\propto n$

This means the ratio of their pressures is equal to the ratio of their number of moles:
$\frac{P_{H_2}}{P_{O_2}}=\frac{n_{H_2}}{n_{O_2}}$

The number of moles of a gas is given by the formula:
$n=\frac{m}{M}$
where $m$ is the mass and $M$ is the molar mass.

For Hydrogen ($H_2$):
Given mass, $m_{H_2}=1\text{g}$
Molar mass of $H_2$, $M_{H_2}=2\text{g/mol}$
So, $n_{H_2}=\frac{1}{2}\text{mol}$

For Oxygen ($O_2$):
Given mass, $m_{O_2}=1\text{g}$
Molar mass of $O_2$, $M_{O_2}=32\text{g/mol}$
So, $n_{O_2}=\frac{1}{32}\text{mol}$

Now, we calculate the ratio of the pressure of hydrogen to oxygen:
$\frac{P_{H_2}}{P_{O_2}}=\frac{1/2}{1/32}=\frac{32}{2}=16$

Therefore, the ratio of hydrogen pressure to oxygen pressure is 16.