the weight of gaseous mixture containing 6.02×10^23 molecules of nitrogen and 3.02×10^23 molecules of sulphur dioxide
Answers
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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: 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 number of atoms.
To calculate the number of moles, we use the equation:
..... (1)
- For Nitrogen:
Number of molecules =
If number of molecules are contained in 1 mole of a compound.
So, number of molecules will be contained in = 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:
Hence, the mass of nitrogen for the given number of molecules is 28 g.
- For sulfur dioxide:
Number of molecules =
If number of molecules are contained in 1 mole of a compound.
So, number of molecules will be contained in = 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:
Hence, the mass of sulfur dioxide for the given number of molecules is 32 g.