Calculate the mass of carbon in a 1-carat diamond that contains 7.56 times 10^22

Question

Calculate the mass of carbon in a 1-carat diamond that contains 7.56 times 10^22 atoms of carbon. G of carbon Calculate the mass of chloroform (CHCl_3, an organic solvent) that contains 1.00 times 10^12 molecules of chloroform, Calculate the number of (a) nitrogen molecules (N_2 molecules) and (b) nitrogen atoms (N atoms) in 0.111 g of nitrogen gas (N_2.) (a) nitrogen molecules (b) nitrogen atoms The mass of a copper coin is 3.20 g. Suppose it were pure copper. (a) How many moles of Cu atoms would the copper contain, given that the molar mass of Cu is 63.55 g/mol? (b) How many Cu atoms are present? (a) moles of Cu atoms Cu atoms Moles, Atoms and Grams

Explanation / Answer

(1)

1 mol of any species has 6.022 * 1023 particles

Molar mass of C = 12 g.

SO, 6.022 * 1023 C atoms are present in 12 g. of C

Then, 7.56 * 1022 C atoms are present in 12 * 7.56 * 1022 / (6.022 * 1023) = 1.51 g. of C

(2) molar mass of chloroform = 119.5 g.

so, 6.022 * 1023 molecuels of chloroform is in 119.5 g. of CHCl3

Then,1.00*1012 molecules of chloroform is present in 1.00*1012*119.5 / (6.022 * 1023) =1.98 * 1012 g. of chloro form.

(3)

Moles of N2 = mass / molar mass = 0.111 / 28 = 0.00396 mol

SO, number of N2 molecules = 0.00396 * 6.022 * 1023 = 2.38 * 1021 molecules of N2

Number of N atoms = 2 * 2.38 *1021 = 4.76 * 1021 atoms of N

(4)

moles of Cu coin = 3.20 / 63.55 = 0.0504 mol

Number of atoms of Cu = 0.0504 * 6.022 * 1023 = 3.04 * 1022 atoms of Cu

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