Chemistry help quick

Question

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 165 mL Cl2(g)165 mL Cl2(g) at 25 °C and 795 Torr795 Torr

Answer 1

MnO₂(s) + 4HCl(aq) ==> MnCl₂(aq) + 2H2O(l) + Cl₂(g) ... balanced equation

molar mass MnO₂ = 86.94 g / mol

molar mass Cl₂ = 70.91 g / mol

Use the ideal gas law to convert 165 ml Cl₂ to moles Cl₂, under the stated conditions:

PV = nRT

n = PV/RT = (795 torr)(0.165 L) / (62.36 Ltorr/Kmol) (298K)

n = 0.00706 moles Cl₂

Use dimensional analysis and the balanced equation to find mass of MnO₂ needed:

0.00706 mols Cl₂ x 1 mol MnO₂ / 1 mol Cl₂ x 86.94 g MnO₂ / mol = 0.614 g MnO₂