How many millimeters of 2.50 M H2SO4 are needed to react completely with 98.5 g of BaO2.
Does anyone know step by step how to do this problem?
You mean milli LITERS, not mm.
a. convert 98.5 g BaO2 to moles dividing by its formula mass
b. check the mole ratio to H2SO4 from the balanced equation. It is 1:1 (making this an easier question!!)
c. multiply answer to a (in moles) by 1L/2.5 mole (the inverse of 2.5 mol / L concentration of the acid)
d. Your answer is now in L, so multiply by 1000 mL/1L to get milliters H2SO4
Comments
You mean milli LITERS, not mm.
a. convert 98.5 g BaO2 to moles dividing by its formula mass
b. check the mole ratio to H2SO4 from the balanced equation. It is 1:1 (making this an easier question!!)
c. multiply answer to a (in moles) by 1L/2.5 mole (the inverse of 2.5 mol / L concentration of the acid)
d. Your answer is now in L, so multiply by 1000 mL/1L to get milliters H2SO4