Question

Which of the following possess highest mass? 

(1) \( 0.2 mol \) of \( CO _{2} \) gas 

(2) \( 2.24 L SO _{2} \) gas at STP 

(3) \( 3.01 \times 10^{23} \) molecules of water 

(4) \( 20 g \) calcium

Answer 1

(1) As given, 0.2 mole of CO₂ gas.

Mass = number of moles x molar mass

1 mole of CO₂ = 44 g

0.2 moles of CO₂ = 44 x 0.2 = 8.8g

(2) As given, 3.01  x 10²³ molecules of water.

1 mole of H₂O contains 6.023 x 10²³ molecules.

6.023 x 10²³ molecules of H₂O = 18g

3.01 x 10²³ molecules of H₂O = \(\frac{18\times3.01\times10^{23}}{6.0253\times10^{23}}\) = 8.99g.

(3) As given, 2.24 L SO₂

1 mole of gas ocupies 22.4 L volume at N.T.P.

22.4 L of SO₂. gas = 64g

2.24 L of SO₂. gas = \(\frac{64\times2.24}{22.4}\) = 6.4g

(4) As given, 20 g calcium

Mass of calcium = 20g

Thus, the highest mass is possesses by 20 g calcium and option(4) is correct.

Comments

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