At which of the following conditions is the d | vedclass

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(C) From the ideal gas equation,$PV = nRT = \frac{m}{M}RT$.Rearranging for density $(d = \frac{m}{V})$,we get $d = \frac{PM}{RT}$.Since $M$ (molar mas

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$0 \, ^\circ C, 1 \, atm$

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(C) From the ideal gas equation,$PV = nRT = \frac{m}{M}RT$.Rearranging for density $(d = \frac{m}{V})$,we get $d = \frac{PM}{RT}$.Since $M$ (molar mass) and $R$ (gas constant) are constant for a given gas,$d \propto \frac{P}{T}$.To maximize density $(d)$,we need the highest pressure $(P)$ and the lowest temperature $(T)$.Comparing the given conditions:$A$: $T = 373 \, K$$B$: $T = 546 \, K$$C$: $T = 273 \, K$$D$: $T = 298 \, K$The lowest temperature is $0 \, ^\circ C$ $(273 \, K)$ at $1 \, atm$ pressure.Therefore,the density is maximum at $0 \, ^\circ C$ and $1 \, atm$.

At which of the following conditions is the density of a gas maximum?

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