an organic compound has an empirical formula ch₂ and a molar mass of 112.21 g/mol. how many h atoms are…

Explanation:

Step1: Calculate the empirical - formula mass

The empirical formula is (CH_2). The molar mass of (C = 12.01\ g/mol) and the molar mass of (H=1.01\ g/mol). The empirical - formula mass (M_{empirical}=(1\times12.01 + 2\times1.01)\ g/mol=14.03\ g/mol).

Step2: Determine the molecular - formula multiplier (n)

The molar mass of the compound (M = 112.21\ g/mol). We use the formula (n=\frac{M}{M_{empirical}}). So, (n=\frac{112.21\ g/mol}{14.03\ g/mol}=8). The molecular formula is ((CH_2)8 = C_8H{16}).

Step3: Calculate the number of moles of the compound in the sample

The mass of the sample (m = 8.61\ g), and the molar mass of the compound (M = 112.21\ g/mol). The number of moles of the compound (n_{compound}=\frac{m}{M}=\frac{8.61\ g}{112.21\ g/mol}=0.0767\ mol).

Step4: Calculate the number of moles of (H) atoms

In one mole of (C_8H_{16}), there are 16 moles of (H) atoms. So, the number of moles of (H) atoms in (0.0767\ mol) of (C_8H_{16}) is (n_H=0.0767\ mol\times16 = 1.2272\ mol).

Step5: Calculate the number of (H) atoms

Using Avogadro's number (N_A = 6.022\times10^{23}\ atoms/mol), the number of (H) atoms (N = n_H\times N_A=1.2272\ mol\times6.022\times10^{23}\ atoms/mol = 7.39\times10^{23}) atoms.

Answer:

(7.39\times 10^{23})