Answer 6 -
Given,
Moles of Fe = 0.82 mol
Moles of O2 = 0.24 mol
moles of Fe2O3 = ?
4 Fe + 3 O2 2 Fe2O3 [BALANCED]
Now, Divide the availabe moles by their stiochiometric coefficients, the one which is smaller is the Limiting reagent.
For Fe = 0.82 mol / 4 = 0.205 mol
For O2 = 0.24 mol /3 = 0.08 mol
So, O2 is the Limiting Reagent.
Using Stiochiometry, it can be analyzed that for 3 moles of O2 , 2 moles of Fe2O3 are produced.
So,
moles of Fe2O3 = 2/3 * moles of O2
moles of Fe2O3 = 2/3 * 0.24 mol
moles of Fe2O3 = 0.16 mol
So, 0.16 mol Fe2O3 is the correct answer
Answer 7 -
Given,
moles of S8 = 0.11 mol
moles of O2 = 0.35 mol
moles of SO3 = ?
S8 + 12 O2 8 SO3 [BALANCED]
Now, Divide the availabe moles by their stiochiometric coefficients, the one which is smaller is the Limiting reagent.
For S8 = 0.11 mol / 1 = 0.11 mol
For O2 = 0.35 mol /12 = 0.029 mol
So, O2 is the Limiting Reagent.
Using Stiochiometry, it can be analyzed that for 12 moles of O2 , 8 moles of SO3 are produced.
So,
moles of SO3 = 8/12 * moles of O2
moles of SO3 = 8/12 * 0.35 mol
moles of SO3 = 0.23 mol
So, 0.23 mol SO3 is the correct answer
12 Ana Cole: Attempt 1 The limiting reactant always has the smallest coefficient in the balanced...
0705 points Question 7 If 0.11 mol Sg reacts with 0.35 mol O2, what is the theoretical yield, in moles, of SO3? - Se + O₂ → SO3 0.65 mol SO3 0.45 mol SO3 0.88 mol SO3 0.23 mol S03 Question 8 0/0.5 points If 3 mol Br2 reacts with 6 mol H2, how many moles of excess reactant are left over? -- Br2 + H2 → ____ HBO 2 mol H2 4 mol Br2 1.5 mol Br2