\(23 \mathrm{~g}\) of \(\mathrm{NO}_{2}\) contains same number of molecules as (a) \(8 \mathrm{~g}\) of oxygen (b) \(28 \mathrm{~g}\) of carbon monoxide (c) \(16 \mathrm{~g}\) of \(\mathrm{SO}_{2}\) (d) \(22 \mathrm{~g}\) of \(\mathrm{CO}_{2}\)

We will use the given mass of NO₂ and its molar mass to calculate moles. Moles of a substance = mass / molar mass. The molar mass of NO₂ is 14 (nitrogen) + 2 x 16 (oxygen) = 46g/mol The moles of 23g NO₂ would be: \(\frac{23}{46}\)

Now we will use the given mass of each substance in the options and find their respective moles to determine which substance has the same number of molecules as the given NO₂. (a) For \(8g\) of oxygen (\(O_{2}\)): molar mass = \(2*16\) = \(32g/mol\), so moles = \(\frac{8}{32}\) (b) For \(28g\) of carbon monoxide (CO): molar mass = \(12+16\) = \(28g/mol\), so moles = \(\frac{28}{28}\) (c) For \(16g\) of \(SO_{2}\): molar mass = \(32+2*16\) = \(64g/mol\), so moles = \(\frac{16}{64}\) (d) For \(22g\) of \(CO_{2}\): molar mass = \(12+2*16\) = \(44g/mol\), so moles = \(\frac{22}{44}\)

The moles of the given NO₂ are \(\frac{23}{46}\). We will compare this value against the moles calculated in step 2 for each substance in the options. (a) The moles of oxygen, \(\frac{8}{32}\), are equal to \(\frac{1}{4}\) (b) The moles of carbon monoxide, \(\frac{28}{28}\), are equal to \(1\) (c) The moles of \(SO_{2}\), \(\frac{16}{64}\), are equal to \(\frac{1}{4}\) (d) The moles of \(CO_{2}\), \(\frac{22}{44}\), are equal to \(\frac{1}{2}\) Since the number of molecules is directly proportional to the number of moles in a substance, comparing the moles will help us determine the substance that has the same number of molecules as the given amount of NO₂. In this case, it is (c) 16g of \(SO_{2}\), which has the same number of moles. Therefore, the correct answer is (c) \(16 \mathrm{~g}\) of \(\mathrm{SO}_{2}\).