2KO2 + H2O → O2 + 2KOH Use the balanced equation to solve the stoichiometry problems below.
a. What mass of KO2 produces 235 g of O2?
b. How many moles of O2 can be removed by 12.3 L of KO2?

Where is the graph ?

Ithink a i think i tried i hope that : )

  the volume of  0.220 m k2s    solution  required  to  completely  react with 175 ml  of 0.115m co(no3)2  calculate the moles  of co(no3)2 =  molarity x volume/1000175 x0.115/1000= 0.02  moleswrite  the reacting  equationk2s(aq)  +  co(no3)2  = 2 kno3(aq)  + cos(s)by  use  of mole ratio between k2s to co(no3)2 which  is  1: 1 the moles of k2s is therefore = 175  x0.115/1000= 0.02  molesvolume = moles/molarity=0.02/0.22=0.09  ml  of k2s