Can anyone help me? Thank you in advance!
1.) Given: 2H2O2=2H2O+O2
a.) What mass of water is produced when 5.0 mol O2 is produced?
2.) Given: 3Fe+4H2O=4H2+Fe3O4
a.) If 625g of Fe3O4 is produced on the reaction how many moles of hydrogen are produced at the same time?
b.) How many moles of iron would be needed to generate 27g of hydrogen?
3.) Given: MnO2+4HCl2=MnCl2+2H20+Cl2
a.) Calculate the mass of MnO2 needed to produced 25 Og of Cl2
b.) What mass of MnCl2 is produced when 0.091g of Cl2 is generated?
Answers & Comments
Answer:
1.) For the reaction 2H2O2=2H2O+O2, the mass of water produced when 5.0 mol of O2 is produced can be calculated as
Moles of O2 produced = 5.0 mol
Moles of water produced = 2 x 5.0 mol = 10.0 mol
Mass of water produced = 10.0 mol x 18.02 g/mol = 180.2 g
2a.) For the reaction 3Fe+4H2O=4H2+Fe3O4, the number of moles of hydrogen produced when 625g of Fe3O4 is produced can be calculated as follows:
Moles of Fe3O4 produced = 625g/231.5 g/mol = 2.684 mol
Moles of hydrogen produced = 4 x 2.684 mol = 10.736 mol
2b.) For the reaction 3Fe+4H2O=4H2+Fe3O4, the number of moles of iron required to produce 625g of Fe3O4 can be calculated as follows:
Moles of Fe3O4 produced = 625g/231.5 g/mol = 2.684 mol
Moles of iron required = 3 x 2.684 mol = 8.052 mol