What is the maximum amount of silver (in grams) that can be plated out of 4.6 LL of an AgNO3AgNO3 solution containing 3.3 %% AgAg by mass? Assume that the density of the solution is 1.01 g/mLg/mL.

153.3 g

Explanation:

Density = 1.01 g/mL

Volume - 4.6 L

1 L = 1000 mL

Volume in mL = 4.6 × 1000 = 4600 mL

Mass = density × volume

         = 1.01 g/mL × 4600 mL

        = 4,646 g

contains 3.3% Ag

Mass of Ag in = 4,646 g × 0.033

                                    = 153.318 g

                                     = 153.3 g

Maximum amount of silver (in grams) that can be plated out is 153.3 g

idk

explanation:

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.