Please see pics. This table looks confusing please help. Consider the balanced chemical reaction below. What is the maximumnumber of grams of Ag that can be produced if 0.570 mol of Zn and 0.691mol of Ag20 react?Zn(s) + Ag,0(s) ZnO(s) + 2 Ag(s)12NEXT >Based on your knowledge of stoichiometry, set up the table below to determine theamounts of each reactant and product after the reaction goes to completion.Zn(s)Ag,0(s)ZnO(s)2 Ag(s)+.Before (mol)0.5700.691XX其减其K 其翼其其其其其其其M 其其M其其X其其其N其丼其N MXNX其其MXN 其N其其其算其ㄨN 其X其NXNXNChange (mol)河 x 河 *其其其 NN 其其 N * *N*M其月NE****After (mol)其其丼X 其其月其其丼+.一 Consider the balanced chemical reaction below. What is the maximumnumber of grams of Ag that can be produced if 0.570 mol of Zn and 0.691mol of Ag20 react?Zn(s) + Ag,0(s)→ ZnO(s) +2 Ag(s)( PREV1.2.Based on the set up your table from the previous step, determine the maximum numberof grams that can be produced.masSag1河NN N 城其ORESET| 12361.45.28 x 10*0.01062.64 x 1014974.537.3%3D

The given chemical reaction is: Zn (s) + Ag2O (s) → ZnO (s) + 2Ag (s) According to stoichiometry here, 1 equivalent of Zn reacted with 1 equivalent of Ag2O to give one equivalent ZnO and two equivalent of Ag. Therefore 0.570 mol of Zn will react with only 0.570 mol of Ag2O to give 0.570 mol of ZnO and (2×0.570) = 1.14 mol of Ag (0.691 − 0.570) = 0.121 mol of Ag2O will remain unreacted. Zn Ag2O ZnO 2 Ag Before (mol) 0.570 0.691 0 0 Change (mol) - 0.570 - 0.570 + 0.570 + 1.14 After (mol) 0 0.121 0.570 1.14The atomic mass of Ag is 107.8 g/mol. Since in the given reaction 1.14 mol of Ag is produced. Therefore, Mass of 1.14 mol of Ag = (1.14 × 107.8) g = 122.89 g of Ag. massAg = 122.89 g ≈ 123 g