Using the reaction: ___ HCl + ___FeI2 + ___ HIO3 → ___ H2O + ICl + ___ FeCl3​ a. balance the chemical equation
b. how many grams of HIO3 is needed to react with 20.0 grams of FeCl3?
c. how many particles of FeI2 is needed to react with 40.0 grams of H2O?
d. how many particles of HCl are needed to produce 2.10 mole of ICl?
e. how many grams of FeCl3 will be produce from 2.03 x 1024 atoms of FeI2?
f. Find the Limiting reactant and excess reactant in FeCl3?
​6g of HIO3
​6g of FeI2
​6g of HCl
g. Find the theoretical yield from FeCl3?
h. What is the percent yield of FeCl3 if the actual yield is 3.0 g?

neutrons are in the middle of the atom and the electrons, which are much smaller.

most likely he is cheating on you

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2