CUET Preparation Today
Calculate the mass of an atom of silver. |
\(1.793 × 10^{–22}g\) \(1.93 × 10^{–22}g\) \(1.0 × 10^{–22}g\) \(2.793 × 10^{–22}g\) |
\(1.793 × 10^{–22}g\) |
The correct answer is option 1. \(1.793 × 10^{–22}g\). \(\text{1 mole of Ag atoms = 108g} \text{ = }6.022\text{ × }10^{23}\) \(6.022\text{ × }10^{23}\text{ atoms of silver have mass = 108g}\) ∴ \(\text{Mass of one atom of silver (Ag) =}\frac{108}{6.022\text{ × }10^{23}}\text{ = }1.793 × 10^{–22}g\) |
