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(D) As we know,$1 \ mol$ of any ideal gas at $STP$ occupies a volume of $22.4 \ L$.Hence,the number of moles of gas $\mu = \frac{44.8}{22.4} = 2 \ mol

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$30R$

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(D) As we know,$1 \ mol$ of any ideal gas at $STP$ occupies a volume of $22.4 \ L$.Hence,the number of moles of gas $\mu = \frac{44.8}{22.4} = 2 \ mol$.Since the volume of the cylinder is fixed,the process is isochoric (constant volume).The heat required at constant volume is given by $\Delta Q_V = \mu C_V \Delta T$.For a monatomic gas,the molar heat capacity at constant volume is $C_V = \frac{3}{2}R$.Substituting the values: $\Delta Q_V = 2 	imes \frac{3}{2}R 	imes 10 = 30R$.

$A$ cylinder of fixed capacity $44.8 \ L$ contains a monatomic gas at standard temperature and pressure $(STP)$. The amount of heat required to raise the temperature of the gas in the cylinder by $10^{\circ}C$ is: ($R =$ universal gas constant)

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