$4 \ g$ of an ideal gas occupies $5.6035 \ L$ of volume at $546 \ K$ and $2 \ atm$ pressure. What is its molecular weight?

For an ideal gas,the volume-temperature graph at constant mass is shown below. What is the correct order of pressure?

The universal gas constant $R$ is defined as:

Match the laws given in List-$I$ with their mathematical forms given in List-$II$.

List-$I$	List-$II$
$(1)$ Boyle's Law	$(A)$ $p \propto T$
$(2)$ Charles's Law	$(B)$ $V \propto n$
$(3)$ Gay-Lussac's Law	$(C)$ $p \propto \frac{1}{V}$
$(4)$ Avogadro's Law	$(D)$ $pV = nRT$
$(5)$ Ideal Gas Equation	$(E)$ $V = k_2T$

$A$ bulb of $1 \, L$ capacity contains $5 \, g$ of ethane. If the pressure increases to $10 \, atm$,what will be the temperature in $^oC$ at which the bulb will burst?

If $P$,$V$,and $T$ represent pressure,volume,and temperature of the gas,the correct representation of Boyle's law is: