Determine the limiting reagent and calculate the theoretical
yield if 0.96 g of benzyltriphenylphosphonium chloride is reacted
with 0.30 mL of cinnamaldehyde.
Which reagent is the limiting reactant when 2.22 mol NaOH and
1.20 mol CO2 are allowed to react?
Which reagent is the limiting reactant when
2.22 and 1.20 are allowed to
react?
NaOH
CO2
Part B. How many moles of Na2CO3 can be produced?
Part C. How many moles of the excess reactant remain after the
completion of the reaction?
1. If you have 10.0g of each reactant, determine the limiting
reagent and the amount of H2O produced.
MnO2 (s) + H2SO4 (l) --->
Mn(SO4)2 (s) + H2O (l)
Can you go over each step?
Determine the limiting reagent and calculate the theoretical
mass of aluminum sulfate formed and the volume of hydrogen gas at
23oC and 752 mm Hg formed if 10.00g of aluminum is
reacted with 10.00g of sulfuric acid. Be sure to show proper
formulas, balanced chemical equations, solution maps and a clear
and complete set-up as instructed including proper dimensional
analysis as appropriate for the problem.
a)Determine the limiting reagent in aspirin synthesis given 3g
of salicylic acid. b)Based on your answer, calculate the maximum
weight of aspirin that you could prepare. c)As is true for most
"organic" reactions the synthesis you do here is an equilibrium
reaction. What steps could you take to improve the yield. d)The
solubility of aspirin in ethanol is approximately 40g/100 mL at
room temperature. If you had a 100% yield, how many milliliters of
ethanol would you need to dissolve...
Determine the limiting reactant (LR) and the
mass (in g) of nitrogen that can be formed from
50.0 g N2O4 and 45.0 g N2H4. Some possibly useful molar masses are
as follows: N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol.
N2O4(l)
+ 2 N2H4(l) → 3 N2(g) + 4 H2O(g)
Balance the following reaction. If we start with 34.1 g of diiodine pentoxide and react with 20.0 g of carbon monoxide, what is the theoretical yield of iodine and what is the limiting reagent? If 20.1 g of iodine is actually obtained, what is the % yield? What volume would the 20.0 g of carbon monoxide occupy at standard temperature and pressure? carbon monoxide + diiodine pentoxide → iodine + carbon dioxide