At a given temperature,the molar mass of gas $A$ is $4$. If it diffuses $3$ times faster than gas $B$,what is the molar mass of gas $B$?

Consider the following statements:
$Statement-I$ : If the intermolecular forces are stronger than thermal energy,the substance prefers to be in a gaseous state.
$Statement-II$ : Among all elements,the total number of elements available as gases at room temperature is $10$.

$A$ and $B$ are ideal gases. The molecular weights of $A$ and $B$ are in the ratio of $1: 4$. The pressure of a gas mixture containing equal weights of $A$ and $B$ is $P \text{ atm}$. What is the partial pressure (in $\text{atm}$) of $B$ in the mixture?

Which one of the following equations represents the variation of viscosity coefficient $(\eta)$ with temperature $(T)$?

If $4 \ g$ of oxygen diffuses through a narrow hole under identical conditions,how many grams of hydrogen will diffuse?

If $1 \ g$ of $CH_4$ gas effuses through a fine hole in $100 \ s$,how many grams of $SO_2$ gas will effuse in $100 \ s$ under the same conditions of temperature and pressure?