What is the mass of silver metal produced from 6.35 g of copper when copper reacts with excess silver nitrate in a single replacement reaction? g?

21.6 grams The balanced equation for the reaction is Cu + 2AgNO3 ==> 2Ag + Cu(NO3)2 So you can easily determine that for each mole of copper used, 2 moles of silver are produced. So let's lookup the atomic weights of copper and silver. Atomic weight copper = 63.546 Atomic weight silver = 107.8682 Moles copper = 6.35 g / 63.546 g/mol = 0.099927611 mol Since we'll produce 2 moles of silver per mole of copper used, we get 0.099927611 mol * 2 = 0.199855223 mol And to get the mass, just multiply by the atomic weight of silver. So 0.199855223 * 107.8682 = 21.55802316 g Finally, round to 3 significant figures, giving 21.6 g.

True, the standard unit for volume is liters which can be represented by either a lower case "l" or a capital "l"