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The empirical formula of a compound used to launch a space shuttle into orbit isNO2 and has a molar mass of 92.0g/mol. The molecular formula of the compound isa) NOAb)N204c)NO2d) none of the above

Sagot :

Let's see first the molar mass of NO2, using the periodic table. You can see that 16 g/mol is the molar mass of oxygen and 14 g/mol is the molar mass of nitrogen. In the formula, there are 2 atoms of oxygen and one atom of nitrogen, so we need to do the algebraic sum to find this molar mass, like this:

[tex]\text{molar mass of NO2=16}\cdot2+14\cdot1=46\frac{g}{mol}[/tex]

But in the problem, they're telling us that the molar mass is 92 g/mol, so we need to multiply each atom by two, because 46 x 2 = 92 g/mol, so the compound would be N2O4. Let's see its molar mass:

[tex]\text{molar mass of N}_2O_4=16\cdot4+14\cdot2=92\text{ }\frac{g}{mol}.[/tex]

The answer is B, N2O4.

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