A signature, written in carbon pencil weighs $1 m g$ . What is the number of carbon atoms present in the signature?

5.02 \times 10^{23}

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5.02 \times 10^{20}

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6.02 \times 10^{20}

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0.502 \times 10^{20}

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Solution

The correct option is C $0.502 \times 10^{20}$
$1 mg = 1 \times 10^{- 3} g$
The number of carbon atoms present in the signature $= \frac{1 \times 10^{- 3} g}{12 g/mol} \times 6.023 \times 10^{23} atoms/mol = 0.502 \times 10^{20} atoms$

Hence the correct option is D.

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A signature, written in carbon pencil weighs 1 mg. What is the number of carbon atoms present in the signature?

The correct option is C 0.502×10201 mg=1×10−3 gThe number of carbon atoms present in the signature =1×10−3 g12 g/mol×6.023×1023 atoms/mol=0.502×1020 atomsHence the correct option is D.

A signature, written in carbon pencil weighs $1 m g$ . What is the number of carbon atoms present in the signature?

The correct option is C $0.502 \times 10^{20}$
$1 mg = 1 \times 10^{- 3} g$
The number of carbon atoms present in the signature $= \frac{1 \times 10^{- 3} g}{12 g/mol} \times 6.023 \times 10^{23} atoms/mol = 0.502 \times 10^{20} atoms$

Hence the correct option is D.