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Question

If 1.8×1019 molecules of NO2 are removed from 10 mg of NO2, how many moles of NO2 are left?

A
3.87×104
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B
1.87×104
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C
1.87×104
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D
2.87×104
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Solution

The correct option is A 1.87×104
First, let's find out the number of molecules present in 10 mg of NO2

The molecular weight of NO2=14 (atomic weight of N )+2×16 (atomic weight of Oxygen)

The molecular weight of NO2=46g

From Avogadro's rule, 1 mole of the NO2 contains 6.022×1023molecules

46g of NO2 contains 6.022×1023molecules

$ 1 g of NO2 contians 6.022×102346g=0.13×1023=0.13×1023molecules
10mg=10×103g=0.13×1023×10×103=0.13×1021=13×1019molecules

10mg of NO2 contains 13×1019molecules

Given that 1.8×1019 molecules were removed from 10 mg of NO2

13×10191.8×1019=(131.8)×1019=11.2.×1019molecules

Now we need to convert these molecules to number of moles

If 6.022×1023 molecules is 1 mole (By Avogadro's rule)

11.2×1019 moelcules contians 1 mole6.022×1023mloecules×11.2×1019molecules

=1.87×104moles

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