_CO2 + _H2O → _C6H12O6 + _O2

For the balanced equation shown below, if the reaction of 40.8 grams of C6H6O3 produces a 39.0% yield, how many grams of H2O would be produced ?

C6H6O3+6O2=>6CO2+3H2O

A hydrocarbon fuel is fully combusted with 18.214 g of oxygen to yield 23.118 g of carbon
dioxide and 4.729 g of water. Find the empirical formula for the hydrocarbon.

For the combustion of sucrose:

C12H22O11 + 12O2 ---> 12CO2 + 11H2O
there are 10.0 g of sucrose and 10.0 g of oxygen reacting. Which is the limiting reagent?

Given the following reaction: Na2S2O3 + AgBr NaBr + Na3[Ag(S2O3)2]

How many moles of Na2S2O3 are needed to react completely with 42.7 g of AgBr?

_SiCl4 + _H2O → _H4SiO4 + _HCl

For the balanced equation shown below, if the reaction of 20.7 grams of CaCO3 produces 6.81 grams of CaO, what is the percent yield?

CaCO3=>CaO+CO2

After combustion with excess oxygen, a 12.501 g of a petroleum compound produced 38.196
g of carbon dioxide and 18.752 of water. A previous analysis determined that the compound
does not contain oxygen. Establish the empirical formula of the compound.

Calculate the number of NaBr formula units formed when 50 NBr3 molecules and 57 NaOH formula units react?

2NBr3 + 3NaOH ---> N2 + 3NaBr + 3HOBr

From the reaction: B2H6 + O2 HBO2 + H2O
How many moles of water are produced from 19.2 g of B2H6?

_Al + _HCl → _AlCl3 + _H2

For the balanced equation shown below, if the reaction of 91.3 grams of C3H6 produces a 81.3% yield, how many grams of CO2 would be produced?

2C3H6+9O2=>6CO2+6H2O

In the course of the combustion analysis of an unknown compound containing only carbon,
hydrogen, and nitrogen, 12.923 g of carbon dioxide and 6.608 g of water were measured.
Treatment of the nitrogen with H2 gas resulted in 2.501 g NH3. The complete combustion of
11.014 g of the compound needed 10.573 g of oxygen. What the compound’s empirical
formula?

Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction:

2Al + 3Cl2 ---> 2AlCl3
How many grams of aluminum chloride could be produced from 34.0 g of aluminum and 39.0 g of chlorine gas?

Calculate the mass (in kg) of water produced from the combustion of 1.0 gallon (3.8 L) of gasoline (C8H18). The density of gasoline is 0.79 g/mL.

_Na2CO3 + _HCl → _NaCl + _H2O + _CO2

For the balanced equation shown below, if the reaction of 0.112 grams of H2 produces 0.745 grams of H2O, what is the percent yield?

Fe3O4+4H2=>3Fe+4H2O

. 12.915 g of a biochemical substance containing only carbon, hydrogen, and oxygen was
burned in an atmosphere of excess oxygen. Subsequent analysis of the gaseous result yielded
18.942 g carbon dioxide and 7.749 g of water. Determine the empirical formula of the
substance.

Suppose 316.0 g aluminum sulfide reacts with 493.0 g of water. What mass of the excess reactant remains?

The unbalanced equation is:

Al2S3 + H2O ---> Al(OH)3 + H2S

KO2 is used in a closed-system breathing apparatus. It removes carbon dioxide and water from exhaled air. The reaction for the removal of water is: KO2 + H2O O2 + KOH. The KOH produced is used to remove carbon dioxide by the following reaction: KOH + CO2 KHCO3.

What mass of KO2 produces 235 g of O2?

_C7H6O2 + _O2 → _CO2 + _H2O

For the balanced equation shown below, if the reaction of 77.0 grams of CaCN2 produces 27.1 grams of NH3, what is the percent yield?

CaCN2+3H2O=>CaCO3+2NH3

33.658 g of oxygen was used to completely react with a sample of a hydrocarbon in a
combustion reaction. The reaction products were 33.057 g of carbon dioxide and 10.816 g of
water. Ascertain the empirical formula of the compound.

In this reaction:

CaCO3 + 2HCl ---> CaCl2 + CO2 + H2O
6.088 g CaCO3 reacted with 2.852 g HCl. What mass of CaCO3 remains unreacted?

Write the balanced chemical equations of the reaction:

C5H12O combusts in air.