Theoretical Yield
2Al + 3Cl2 → 2AlCl3
Calculate the theoretical yield of aluminum chloride (in grams) that can be produced from 10.00 grams of aluminum metal.
49.418 g AlCl3
A reaction with a calculated yield of 9.23 g produced 7.89 g of product. What is the percent yield for this reaction?
85.5%
2NO + O2 → 2NO2
2 moles of NO will react with ______ mole(s) of O2 to produce ______ mole(s) of NO2
2 moles of NO will react with 1 mole(s) of O2 to produce 2 mole(s) of NO2
___HCl + ___NaOH → ___NaCl + ___H2O
HCl + NaOH → NaCl + H2O
Ca(OH)2 + 2HCl → 2H2O + CaCl2
How many moles of Ca(OH)2 are required to react with 6.4 moles of HCl?
3.2 mol Ca(OH)2
Cl2O7 + H2O → 2HClO4
An initial mass of 4.00 grams of dichlorine heptoxide (Cl2O7) was used to synthesize a sample of perchloric acid (HClO4). Calculate the theoretical yield, given this information.
4.394 g HClO4
5.96 g of ammonia (17.031 g/mol) react completely according to the following reaction:
2NH3 + CO2 → CN2OH4 + H2O
The theoretical yield is 17.4 g. If 13.74 g of urea (CN2OH4 60.056 g/mol) are produced, what is the percent yield for this reaction?
79.0%
2C10H22 + 31O2 → 20CO2 + 22H2O
How many moles of CO2 are produced if 5.0 moles of C10H22 react with an excess of O2?
50 mol CO2
___H3PO4 + ___KOH → ___K3PO4 + ___H2O
H3PO4 + 3KOH → K3PO4 + 3H2O
2C2H2 + 5O2 → 4CO2 + 2H2O
How many moles of O2 are required to produce 8.2 moles of H2O?
20.5 mol O2
2C4H10 + 13O2 → 8CO2 + 10 H2O
Calculate the mass of carbon dioxide (in grams) that can be produced from 20.00 grams of butane liquid.
60.58 g CO2
15.4 g of methanol (CH3OH 32.042 g/mol) reacts completely according to the following reaction:
CH3OH → CH2O + H2
If 12.35 g of formaldehyde (30.026 g/mol) is produced, what is the percent yield for this reaction?
Theoretical Yield = 14.4 g
Percent Yield = 85.8%
C3H8 + 5O2 → 3CO2 + 4H2O
How many moles of oxygen react with 11 moles of C3H8?
55 moles O2
___Rb + ___RbNO3 → ___Rb2O + ___N2
10Rb + 2RbNO3 → 6Rb2O + N2
2C2H2 + 5O2 → 4CO2 + 2H2O
How many moles of H2O are produced when 10.5 moles of O2 react?
4.2 mol H2O
_V + _O2 → _V2O3
Balance the reaction. Then, calculate the theoretical yield of vanadium(III) oxide, assuming you begin with 200.00 grams of vanadium metal.
4V + 3O2 → 2V2O3
294.23 g V2O3
85.4 g of chlorine (70.91 g/mol) reacts completely according to the following reaction:
P4 + _Cl2 → _PCI3
If 104 g of phosphorus trichloride (137.3 g/mol) is produced, what is the percent yield for this reaction?
P4 + 6Cl2 → 4PCI3
Theoretical Yield = 110 g
Percent Yield = 94.5%
___AlF3 + ___O2 → ___Al2O3 + ___F2
20 moles of AlF3 will produce ______ moles of F2
4AlF3 + 3O2 → 2Al2O3 + 6F2
30 moles F2
___ Al + ___ S8 → ___ Al2S3
16Al + 3S8 → 8Al2S3
_C3H8 + _O2 → _CO2 + _H2O
If 12 moles of carbon dioxide are formed, how many moles of C3H8 (propane) were burned?
C3H8 + 5O2 → 3CO2 + 4H2O
4 mol C3H8
_KI + _H2O + _KMnO4 → _I2 + _ MnO2 + _KOH
Calculate the mass of manganese(IV) oxide that can be synthesized from 15.00 grams of potassium iodide.
6KI + 4H2O + 2KMnO4 → 3I2 + 2MnO2 + 8KOH
2.618 g MnO2
Al(OH)3 + _HCl → AlCl3 + _H2O
If you start with 50.3 g of Al(OH)3 and you isolate 39.5 g of AlCl3, what is the percent yield?
Al(OH)3 + 3HCl → AlCl3 + 3H2O
Theoretical Yield = 86.98 g
Percent Yield = 49.94%
___NH3 + ___O2 → ___N2 + ___H2O
a. 20 moles of NH3 are needed to produce ______ moles of H2O. b. How many moles of N2 will be produced if 3.5 moles of O2 react?
4NH3 + 3O2 → 2N2 + 6H2O
a. 30 mole H2O
b. 2.33 mol N2
___ Ca3(PO4)2 + ___ SiO2 + ___ C → ___ CaSiO3 + ___ CO + ___ P
Ca3(PO4)2 + 3SiO2 + 5C → 3CaSiO3 + 5CO + 2P
_AgNO3 + _MgBr2 → _AgBr + _Mg(NO3)2
If 3.13 moles of MgBr2 react completely with excess AgNO3, how many grams of AgBr are formed?
2AgNO3 + MgBr2 → 2AgBr + Mg(NO3)2
1175.45 g AgBr