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12 g of carbon contains 6.02times 10^23 atoms. Which expression is used to calculate the mass of one atom of carbon? Tick (v) one box. (12)/(6.02times 10^23) square (6.02times 10^23)/(12) 12times 6.02times 10^23 square

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12 g of carbon contains 6.02times 10^23 atoms. Which expression is used to calculate the mass of one atom of carbon? Tick (v) one box. (12)/(6.02times 10^23) square (6.02times 10^23)/(12) 12times 6.02times 10^23 square

12 g of carbon contains 6.02times 10^23 atoms. Which expression is used to calculate the mass of one atom of carbon? Tick (v) one box. (12)/(6.02times 10^23) square (6.02times 10^23)/(12) 12times 6.02times 10^23 square

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HedyddExpert · Tutor for 3 years

Answer

\( \frac{12}{6.02 \times 10^{23}} \)

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## Step1:<br />First, we need to understand that the equation to find the mass of single atom of Carbon is given as <br />'\(\text{Mass of atom} = \frac{\text{Total mass of atoms}}{\text{Number of Atoms}} \)'. Where, given,<br />### Total mass of carbon = 12 g<br />### Number of Carbon atoms = \( 6.02 \times 10^{23} \)<br /><br />## Step2: <br />If we substitute these values into the equation that we formed in the previous step then the input would be,<br /><br />### ***Mass of atom*** \(= \frac{\text{Total mass of atoms}}{\text{Number of Atoms}} = \frac{12}{6.02 \times 10^{23}} \)<br /><br />Comparing this result with the given options:<br />\( \frac{12}{6.02 \times 10^{23}} \), "\( \frac{6.02 \times 10^{23}}{12} \)" and "\(( 12 \times 6.02 \times 10^{23})\)",<br />We observe that the first option matches with our calculated result making "\(\frac{12}{6.02 \times 10^{23}}\)" the correct answer.
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