The weight of a gaseous mixture containing $12.044\times {10}^{23}$ atoms of He and $6.022\times {10}^{23}$ molecules of hydrogen is _____________ g.

 

Given, number of He atoms = $12.044\times {10}^{23}$

Number of H atom = $6.022\times {10}^{23}$

Formula/concept used: Stoichiometric calculation

Detailed solution: Molar mass of He = 4g

Molar mass H = 2g

Moles of He = 2

Moles of H = 1

Weight of gaseous mixture = 2(4) + 1(2) = 10g

Therefore, the weight of the mixture is 10g.