$\begin{array}{1,1}(a)\;489.23mm,260.77mm\\(b)\;543.1mm,432.1mm\\(c)\;249.33mm,146.21mm\\(d)\;211.3mm,423.1mm \end {array}$

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Given

Weight of gas A = 0.50 g

Molecular weight of gas A = 60

Weight of gas B = 0.2 g

Molecular weight of gas B = 45

Pm = 750mm

From Daltons's law of partial pressure

$P'_A = P_m\times$ mole fraction of A

$ = 750\times{\large\frac{\frac{0.5}{60}}{(\large\frac{0.5}{60})+(\large\frac{0.2}{45})}}$

$ = 489.23 mm$

Now $P_m = P'_A +P'_B$

$P'_B = P_m - P'_A $

=750 - 489.23 = 260.77 mm

Hence answer is (a)

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