Question

the weight of gaseous mixture containing 6.02×10^23 molecules of nitrogen and 3.02×10^23 molecules of sulphur dioxide

Answer 1

6.02 × 10^23 molecules of N2 = 1mole of N2
&
3.02×10^23molecules of SO2=1/2moles of SO2

So mass of 1mole of N2 =2×14=28g
and mass of 1/2 moles of SO2 =1/2×(32+16×2)
=1/2×64 =32g

So total weight of the gaseous mixture
=28+32=60g

HOPE IT HELPS..... :-)

Answer 2

Answer: The mass of nitrogen and sulfur dioxide for the given number of molecules is 28 g and 32 g respectively.

Explanation:

According to mole concept:

1 mole of an element contains $6.022\times 10^{23}$ number of atoms.

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$  ..... (1)

• For Nitrogen:

Number of molecules = $6.02\times 10^{23}$

If $6.022\times 10^{23}$ number of molecules are contained in 1 mole of a compound.

So, $6.02\times 10^{23}$ number of molecules will be contained in = $\frac{1mol}{6.022\times 10{23}}\times 6.02\times 10^{23}=1mol$ of nitrogen.

Using equation 1, we get:

Moles of nitrogen = 1 mole

Molar mass of nitrogen = 28 g/mol

Putting values in equation 1, we get:

$1mol=\frac{\text{Mass of nitrogen}}{28g/mol}\\\\\text{Mass of nitrogen}=28g$

Hence, the mass of nitrogen for the given number of molecules is 28 g.

• For sulfur dioxide:

Number of molecules = $3.02\times 10^{23}$

If $6.022\times 10^{23}$ number of molecules are contained in 1 mole of a compound.

So, $3.02\times 10^{23}$ number of molecules will be contained in = $\frac{1mol}{6.022\times 10{23}}\times 3.02\times 10^{23}=0.5mol$ of sulfur dioxide.

Using equation 1, we get:

Moles of sulfur dioxide = 0.5 mole

Molar mass of sulfur dioxide = 64 g/mol

Putting values in equation 1, we get:

$0.5mol=\frac{\text{Mass of sulfur dioxide}}{64g/mol}\\\\\text{Mass of sulfur dioxide}=32g$

Hence, the mass of sulfur dioxide for the given number of molecules is 32 g.