Consider the unbalanced equation: MgCl2(aq) + AgNO3(aq) AgCl(s) + Mg(NOJ2(aq) → a) If 5.00 g MgCl2 and 5.00 g AgNOs are allowed to react, how many grams of AgCl would be produced? b) Which reactant is not totally consumed by the reaction? How much remains (g)?

Heya dearfirst love doesn't matter what the it's just happen so we cannot say that minor in love with someone over 18 years old

The total number of electrons is 14

  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