Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq)HCl(aq), as described by the chemical equation MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+ Cl2(g) MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+ Cl2(g) How much MnO2(s)MnO2(s) should be added to excess HCl(aq)HCl(aq) to obtain 235 mL Cl2(g)235 mL Cl2(g) at 25 °C and 805 Torr805 Torr?

0.887 g of should be added to excess HCl(aq).

Explanation:

According to ideal gas equation:

P = pressure of gas = 805 torr = 1.06 atm  (760torr=1atm)

V = Volume of gas = 235 ml = 0.235 L

n = number of moles = ?

R = gas constant =

T =temperature =

According to stoichiometry:

1 mole of chlorine is produced by = 1 mole of

Thus 0.0102 moles of chlorine is produced by = moles of

Mass of =

0.887 g of should be added to excess HCl(aq).

the dependant variable is spilled water

the independent is the heat

2b2t

explanation:

2b2t