Multiple choice

There are $6.02 \times {10^{22}}$ molecules each of ${N_2},\,\,{O_2}\,\,{\text{and}}\,\,{H_2}$ which are mixed together at 760 mm and 273 K. The mass of total mixture in grams is

  1. 6.2 gm

  2. 4.12 gm

  3. 3.09 gm

  4. 7 gm
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation

The number of molecules 6.02 * 10^22 is 0.1 moles. Each gas (N2, O2, H2) has 0.1 moles. The molar masses are 28, 32, and 2 g/mol respectively. Total mass = 0.1(28 + 32 + 2) = 0.1(62) = 6.2 grams.

AI explanation

To find the mass of each gas, divide the given number of molecules by Avogadro's number, 6.02 x 10^23, to get 0.1 moles per gas. Multiplying 0.1 moles by their respective molar masses gives 2.8 g for N2, 3.2 g for O2, and 0.2 g for H2. The total mass of the mixture is the sum of these individual masses, 2.8 + 3.2 + 0.2, which equals 6.2 gm.

Keep practicing — related questions