Question #315800

Consider the reaction MnO2 + 4HCI → MnCl2 + Cl2 + 2H2O. If the both the


reactants have a mass of 100 grams, which of the two will be used up first? How


many grams of MnCl2 will be produced after the reaction? (MnO2 =


86.94 g/mol, HC1 = 36.46 g/mol, MnCl2 = 125.8 g/mol)

1
Expert's answer
2022-03-23T09:54:02-0400

Calculate ν:\nu:

ν(MnO2)=m(MnO2)/M(MnO2)=100g/(86.94g/mol)=1.15mol\nu(MnO_2) =m(MnO_2)/M(MnO_2)=100g/(86.94 g/mol)=1.15 mol

ν(HCl)=m(HCl)/M(HCl)=100g/(36.46g/mol)=2.74mol\nu(HCl) =m(HCl)/M(HCl)=100g/(36.46 g/mol)=2.74 mol


1 mol of MnO2MnO_2 reacts with 4 mol of HClHCl , 1.15 mol of MnO2MnO_2 reacts with 4.6 mol of HClHCl

MnO2MnO_2 in excess

HCl will be used up first - it limiting reagent.


According to the equation we get 1/4 mol of MnCl2MnCl_2 from 1 mol of HCl, therefore:

m(MnCl2)=ν(MnCl2)M(MnCl2)=1/4ν(HCl)M(MnCl2)=m(MnCl_2)=\nu(MnCl_2)\cdot M(MnCl_2)=1/4\cdot \nu(HCl)\cdot M(MnCl_2)=

=0.252.74mol125.8g/mol=86.17g=0.25\cdot 2.74 mol\cdot 125.8 g/mol=86.17g


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