Question

Determine the theoretical yield (in grams) of AlBr3 when 5.00 grams of Al and excess Br2 are reacted according to the reaction below. Molar mass of AlBr3 is 266.68 g/mol.

2Al(s) + 3Br2(l) ⟶ 2AlBr3(s)

Answer #1

1- Using the balanced equation given below, calculate the number
of grams of Br 2 needed to react with exactly 53.8 g of Al.
2Al (s) + 3Br2 = 2AlBr3(s)
2- Calculate the number of moles of CO2 generated by the
reaction given below when 6.78 g of CaCO3 is heated.
CaCO3 = CaO + CO2(g)
3- Calculate the percent yield of the product if the actual
yield is 22.45 g of AlBr3

28. Determine the theoretical yield of HCl if 30.0 g of BCl3 and
32.5 g of H2O are reacted according to the following balanced
reaction. A possibly useful molar mass is BCl3 = 117.2 g/mol.
BCl3(g) + 3H2O(l) 3H3BO3(s) + 3HCl(g)
29. Which should give the most vigorous reaction when dropped in
water?
(A). Mg (B). C (C). Na (D). Ca
(E). U
30. Lithium and nitrogen react to produce lithium nitride:
6Li(s) + N2(g) --> 2Li3N(s) How many...

For the reaction shown, compute the theoretical yield of the
product in grams for each of the following initial amounts of
reactants. 2Al(s)+3Cl2(g)→2AlCl3(s)
Part B: 5.5 g Al; 19.8 g Cl2
Part C: 0.439 g Al; 2.29 g Cl2
Express your answers using three significant figures.
Thank you! :)

a) Determine the mass (in grams) of bromine that will result in
a change in energy of -2.58 kJ when bromine reacts with excess
potassium iodide according to the following balanced thermochemical
equation:
2KI(s) + Br2(l) → 2KBr(s) +
I2(s) ΔHr° =
-131.80 kJ
b) Using the enthalpies of formation given below, Calculate the
amount of heat absorbed/released (in kJ) when 8.39 grams of
SO2 are produced via the above reaction.
2H2S(g) + 3O2(g) → 2SO2(g) +
2H2O(l)
H2S (g): -20.60...

Determine the limiting reagent and theoretical yield if 1.2 g of
salicylic acid (molar mass: 138.12 = g/mol) is reacted with 3.0 mL
of acetic anhydride (molar mass = 102.09 g/mol and p = 1.082
g/mL).

Calculate the percent yield if 31.6 grams of C4H8Br2 are
produced when 10.0 grams of C4H8 are reacted with excess Br2. The
reaction is C4H8 + Br2 ---> C4H8Br2

Determine the theoretical yield of CO2 (in grams) for the
reaction below if you have 18.0 g of C2H4 and 45.0 g of O2.
C2H4(g) + 3 O2(g)à2 CO2(g) + 2
H2O(l)

A 2.25 gram sample of zinc metal reacts with 5.00 grams of
hydrochloric acid to give zinc chloride and hydrogen gas according
the blanced equation:
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) Molar mass ZnCl2: 136.28
g/mol
a. What is the limiting reactant?
b. What mass of ZnCl2 can be formed? (This is called the
theoretical yield.)

For the reaction shown, compute the theoretical yield of the
product in grams for each of the following initial amounts of
reactants. 2Al(s)+3Cl2(g)→2AlCl3(s) 1.) 5.5 gAl; 19.8 gCl2 2.)
0.439 gAl; 2.29 gCl2

Benzene,C6H6(ℓ), reacts with bromine,
Br2 to form bromobenzene,
C6H5Br(ℓ) as described below
C6H6(ℓ)
+ Br2(ℓ) →
C6H5Br(ℓ)
+ HBr(g)
Calculate the amount of bromobenzene,
C6H5Br(ℓ), in grams that can be produced from
reaction of 30.0 g of C6H6 and 50.0 g
Br2?
Molar Mass C6H6 = 78.11 g/mol
Molar Mass Br2 = 159.8 g/mol Molar
Mass C6H5Br = 157.0 g/mol
Hint: This is a limiting reactant problem.

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