A mixture of 4g of hydrogen and 8 g of helium at NPT has a density about

0.22 k g / m^{3}

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0.62 k g / m^{3}

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1.12 k g / m^{3}

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0.13 k g / m^{3}

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Solution

The correct option is D $0.13 k g / m^{3}$
Average molecular mass of the mixture= $\frac{m_{1} M_{1} + m_{2} M_{2}}{m_{1} + M_{2}} = \frac{(4) (2) + (8) (4)}{4 + 8} = 3.33 g / m o l$
From ideal gas law we know, $P M_{m i x} = ρ R T$
$⟹ ρ = \frac{P M_{m i x}}{R T} = 0.13 k g / m^{3}$

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A mixture of 4g of hydrogen and 8 g of helium at NPT has a density about

The correct option is D 0.13kg/m3Average molecular mass of the mixture=m1M1+m2M2m1+M2=(4)(2)+(8)(4)4+8=3.33g/molFrom ideal gas law we know, PMmix=ρRT⟹ρ=PMmixRT=0.13kg/m3

The correct option is D $0.13 k g / m^{3}$
Average molecular mass of the mixture= $\frac{m_{1} M_{1} + m_{2} M_{2}}{m_{1} + M_{2}} = \frac{(4) (2) + (8) (4)}{4 + 8} = 3.33 g / m o l$
From ideal gas law we know, $P M_{m i x} = ρ R T$
$⟹ ρ = \frac{P M_{m i x}}{R T} = 0.13 k g / m^{3}$