your claim. 9. How heavy (in grams) will 6.14times 10^25 atoms of gold be? 10. How many carbon atoms are in 100 grams of glucose( C_(6)H_(12)O_(6))

9. To find the mass of $6.14\times 10^{25}$ atoms of gold, we need to use Avogadro's number, which is $6.022\times 10^{23}$ atoms/mol. <br /><br />First, we need to find the molar mass of gold (Au), which is 197.0 g/mol.<br /><br />Next, we can calculate the number of moles of gold atoms:<br />Number of moles = $\frac{6.14\times 10^{25}}{6.022\times 10^{23}}$<br /><br />Now, we can calculate the mass of gold atoms:<br />Mass = Number of moles * Molar mass of gold<br />Mass = $\frac{6.14\times 10^{25}}{6.022\times 10^{23}}$ * 197.0 g/mol<br /><br />After performing the calculation, we find that the mass of $6.14\times 10^{25}$ atoms of gold is approximately 2.04 x 10^6 grams.<br /><br />10. To find the number of carbon atoms in 100 grams of glucose ($C_{6}H_{12}O_{6}$), we need to use the molar mass of glucose, which is 180.16 g/mol.<br /><br />First, we can calculate the number of moles of glucose:<br />Number of moles = $\frac{100}{180.16}$<br /><br />Next, we can calculate the number of carbon atoms in one mole of glucose:<br />Number of carbon atoms in one mole of glucose = 6<br /><br />Finally, we can calculate the total number of carbon atoms in 100 grams of glucose:<br />Total number of carbon atoms = Number of moles * Number of carbon atoms in one mole of glucose<br />Total number of carbon atoms = $\frac{100}{180.16}$ * 6<br /><br />After performing the calculation, we find that there are approximately 3.33 moles of carbon atoms in 100 grams of glucose.