(i) 16 g of CO: The molar mass of CO (Carbon Monoxide) is 28 g/mol. So, 16 g of CO is 16/28 = 0.57 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 0.57 mol of CO contains 0.57 x 6.022 x 10^23 = 3.43 x 10^23 molecules.

(ii) 28 g of N2: The molar mass of N2 (Nitrogen) is 28 g/mol. So, 28 g of N2 is 28/28 = 1 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 1 mol of N2 contains 1 x 6.022 x 10^23 = 6.022 x 10^23 molecules.

(iii) 14 g of N2: The molar mass of N2 (Nitrogen) is 28 g/mol. So, 14 g of N2 is 14/28 = 0.5 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 0.5 mol of N2 contains 0.5 x 6.022 x 10^23 = 3.011 x 10^23 molecules.

(iv) 1.0 g of H2: The molar mass of H2 (Hydrogen) is 2 g/mol. So, 1 g of H2 is 1/2 = 0.5 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 0.5 mol of H2 contains 0.5 x 6.022 x 10^23 = 3.011 x 10^23 molecules.

So, 16 g of oxygen has the same number of molecules as 28 g of N2, but not the same as 16 g of CO, 14 g of N2, or 1.0 g of H2.

Question

(i) 16 g of CO: The molar mass of CO (Carbon Monoxide) is 28 g/mol. So, 16 g of CO is 16/28 = 0.57 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 0.57 mol of CO contains 0.57 x 6.022 x 10^23 = 3.43 x 10^23 molecules.

(ii) 28 g of N2: The molar mass of N2 (Nitrogen) is 28 g/mol. So, 28 g of N2 is 28/28 = 1 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 1 mol of N2 contains 1 x 6.022 x 10^23 = 6.022 x 10^23 molecules.

(iii) 14 g of N2: The molar mass of N2 (Nitrogen) is 28 g/mol. So, 14 g of N2 is 14/28 = 0.5 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 0.5 mol of N2 contains 0.5 x 6.022 x 10^23 = 3.011 x 10^23 molecules.

(iv) 1.0 g of H2: The molar mass of H2 (Hydrogen) is 2 g/mol. So, 1 g of H2 is 1/2 = 0.5 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 0.5 mol of H2 contains 0.5 x 6.022 x 10^23 = 3.011 x 10^23 molecules.

So, 16 g of oxygen has the same number of molecules as 28 g of N2, but not the same as 16 g of CO, 14 g of N2, or 1.0 g of H2.

Knowee AI · Accepted Answer

(i) 16 g of CO: The molar mass of CO (Carbon Monoxide) is 28 g/mol. So, 16 g of CO is 16/28 = 0.57 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 0.57 mol of CO contains 0.57 x 6.022 x 10^23 = 3.43 x 10^23 molecules.

(ii) 28 g of N2: The molar mass of N2 (Nitrogen) is 28 g/mol. So, 28 g of N2 is 28/28 = 1 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 1 mol of N2 contains 1 x 6.022 x 10^23 = 6.022 x 10^23 molecules.

(iii) 14 g of N2: The molar mass of N2 (Nitrogen) is 28 g/mol. So, 14 g of N2 is 14/28 = 0.5 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 0.5 mol of N2 contains 0.5 x 6.022 x 10^23 = 3.011 x 10^23 molecules.

(iv) 1.0 g of H2: The molar mass of H2 (Hydrogen) is 2 g/mol. So, 1 g of H2 is 1/2 = 0.5 mol. According to Avogadro's law, one mole of any substance contains 6.022 x 10^23 molecules. So, 0.5 mol of H2 contains 0.5 x 6.022 x 10^23 = 3.011 x 10^23 molecules.

So, 16 g of oxygen has the same number of molecules as 28 g of N2, but not the same as 16 g of CO, 14 g of N2, or 1.0 g of H2.

16 g of oxygen has same number of molecules as in 1 point(i) 16 g of CO(ii) 28 g of N2(iii) 14 g of N2(iv) 1.0 g of H2

Question

Solution

Similar Questions

Upgrade your grade with Knowee