5. How many grams of silver will be formed from 0.5mol magnesium? underline ( )Mg(s)+underline ( )AgNO_(3)(aq)arrow underline ( )Ag(s)+underline ( )Mg(NO_(3))_(2)(aq)

To determine how many grams of silver will be formed from 0.5 mol of magnesium, we need to use stoichiometry based on the balanced chemical equation:<br /><br />\[ \text{Mg}(s) + 2\text{AgNO}_3(aq) \rightarrow 2\text{Ag}(s) + \text{Mg(NO}_3\text{)}_2(aq) \]<br /><br />From the balanced equation, we see that 1 mole of magnesium (Mg) produces 2 moles of silver (Ag).<br /><br />Given:<br />- 0.5 moles of Mg<br /><br />Using the stoichiometric ratio:<br />\[ \text{Moles of Ag} = 0.5 \text{ moles of Mg} \times \frac{2 \text{ moles of Ag}}{1 \text{ mole of Mg}} = 1 \text{ mole of Ag} \]<br /><br />Now, we need to convert moles of silver to grams. The molar mass of silver (Ag) is approximately 107.87 g/mol.<br /><br />\[ \text{Mass of Ag} = 1 \text{ mole of Ag} \times 107.87 \text{ g/mol} = 107.87 \text{ grams of Ag} \]<br /><br />Therefore, 107.87 grams of silver will be formed from 0.5 moles of magnesium.