Saved Bookmarks
| 1. |
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) 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. |
|