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Calculate the volume of chlorine gas at STP that is required to completely react with 3.50 g of silver, using the following equation:2Ag(s) + C12(9)
-2AgCl(s).

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Eduard22sly

The volume of chlorine gas at STP required for the reaction is 0.363 L (i.e 363 mL)

How to determine the mole of Silver, Ag

  • Mass of Ag = 3.5 g
  • Molar mass of Ag = 108 g/mol
  • Mole of Ag =?

Mole = mass / molar mass

Mole of Ag = 3.5 / 108

Mole of Ag = 0.0324 mole

How to determine the mole of Cl₂ that reacted

Balanced equation

2Ag + Cl₂ —> 2AgCl

From the balanced equation above,

2 mole of Ag reacted with 1 mole of Cl₂.

Therefore,

0.0324 mole of Ag will react with = 0.0324 / 2 = 0.0162 mole of Cl₂

How to determine the volume of Cl₂

  • Number of mole (n) = 0.0162 mole
  • Pressure (P) = STP = 1 atm
  • Temperature (T) = STP = 273 K
  • Gas constant (R) = 0.0821 atm.L/Kmol
  • Volume (V) =?

The volume of chlorine gas, Cl₂ required for the reaction can be obtained by using the ideal gas equation as follow:

PV = nRT

1 × V = 0.0162 × 0.0821 × 274

V = 0.363 L or  363 mL

Learn more about stoichiometry:

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