If $2 \, \text{moles}$ of an ideal gas occupy a volume of $44.8 \, L$ at a temperature of $546 \, K$,what will be the pressure in $atm$?

$A$ mass of gas occupies $11.2 \ dm^3$ at $105 \ kPa$. What is its volume if the pressure is increased to $210 \ kPa$ at constant temperature (in $dm^3$)?

Which of the following represents the correct relationship between the change in density of an ideal gas and the change in temperature?

In order to increase the volume of a gas by $10 \%$ at constant temperature,the pressure of the gas should be:

The vapors of $1 \ g$ of an element occupy $2.5625 \ L$ exerting a pressure of $0.5 \ atm$ at $1000 \ K$. What is the molar mass (in $g \ mol^{-1}$) of the element? (Assume vapors follow ideal gas equation. Given $R=0.082 \ L \ atm \ mol^{-1} \ K^{-1}$)

If $4 \ g$ of $O_2$ and $2 \ g$ of $H_2$ are filled in a $1 \ L$ bulb at $0 \ ^oC$,the total pressure of the mixture will be...... (in $atm$)