Question

can you please answer all of the parts

d slf Section B: Show all your calculation steps with conversion factors formula of reactants and products, setup with units, calculator value and correct significant figures. Calculation of molar mass should be shown when needed. All atomic mass of elements are up to two decimals as given in the periodic table. Following Reaction is given when zinc reacts with sulfur to form ZnS. 1 Zn (s)+ S(s) ZnS Determine the limiting reactant when 12.72 g of Zn react with 10.90 g of sulfur (S) to produce ZnS? Show all calculation steps by using conversion factors and units. (4 pt) Srep 1: Mole of ZnS from (g) of Zn Step 2: Mole of ZnS from (g) ofS mole of ZnS produced is Limiting reactant is: Calculate the theoretical yield (mass) of ZnS formed in the above reaction. Show all steps of calculation by using conversion factors and units. (2 pts) b) If the actual mass of ZnS produced is 14.51 g. Calculate percent yield of this reaction (2pts) Show Formula and calculation Steps

Answer 1

Zn (s) + S (s) ~ Zns mole of Zn = w Gym = 12.72g 65g/mol - 0.19 mol mole of s = 10.90g 32 g/mol = 0.34 mol Rati Ralso of coefficient of an tos - Ratio of the moles of an tos I molzn = 0.19 mol of an I mots & mot of s x mol of = 0.19 mot of zn. So, moles of s required is 0.19 mol but we have 0.34 mol ons which means in excess. That's why Limiting reagent is zn. Ratio of coefficient of an to Ens = Ratio of the moles of an tozns Imolan – 0.19 mol of n. I mot ens a mol of zus. mot of ans - d. 19 mol w of ens = 0.19 molx (65+ 32) g/mol = 18139 [Wans & 18 g/ Given ens produced & 14.51g percent yield actual yield theoretical yield X100 14.51 g x100 18 9 0.81 X 100 percent yield = 818