Stoichvbdsj

What is the study of the mass relationships among reactants and products in a chemical reaction?

reaction stoichiometry

How many moles of Ag can be produced if 350 g of Cu are reacted with excess AgNO3 according to the equation Cu(s) + 2AgNO3 (aq) --> 2Ag(s) + Cu(NO3)2(aq)

10.94 mols

for the reaction represented by the equation 2H2 + O2 --> 2H2O how many grams of water are produced from 6 mol of oxygen

108 g

for the reaction represented by the equation 2H2 + O2 --> 2H2O, how many moles of water can be produced from 6.0 mol of water

12 mol

for the reaction represented by the equation 2Na + 2H2O --> 2NaOH + H2 , how many grams of sodium hydroxide are produced from 3.0 mol of sodium with an excess of water

120 g

for the reaction represented by the equation C12 + 2KBr --> 2KCl + Br2, how many grams of potassium chloride can be produced from 300 g of chlorine and potassium bromide?

188 g

in the reaction represented by the equation N2 + 3H2 --> 2NH3 , what is the mole ratio of nitrogen to ammonia

1:2

Ozone, O3, is produced by the reaction represented by the following equation: NO2(g)+O2(g)-->NO(g)+O3(g) What mass of ozone will form from the reaction 2.0 g of NO2 in a car's exhaust and excess oxygen?

2.1 g O3

For the reaction represented by the equation C + 2H2 ---> CH4, how many moles of hydrogen are required to produce 10 mol of methane, CH4?

20 mol

for the reaction represented by the equation SO3 + H20 --> H2SO4 , how many grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid in excess of water

320 g

(SA) What mass in grams of sodium hydroxide is produced if 20 g of sodium metal react with excess water according to the chemical equation 2Na(s) + 2H2O(l) --> 2NaOH(aq) + H2(g)

34.80 g

for the reaction represented by the equation 2Na + 2H2O --> 2NaOH + H2 , how many grams of hydrogen are produced if 120 g of sodium and 80 g of water are available

4.5 g

In the equation 2KCIO3 --> 2KCI +3O2 how many moles of oxygen are produced when 3.0 mol of KCIO3 decompose completely

4.5 mol

(SA) What mass in grams of hydrogen gas is produced if 20 mol of Zn are added to excess hydrochloric acid according to the equation Zn(s) + 2HCI(aq) --> ZnCI2(aq) + H2(g)

40g

for the reaction represented by the equation CH4 + 2O2 --> 2H2O + CO2, calculate the percent yield of carbon dioxide if 1000 g of methane react with excess oxygen to produce 2300 g of carbon dioxide

83.88%

for the reaction represented by the equation Cl2 + 2KBr --> 2KCl + Br2 , calculate the percentage yield if 200 g of chlorine react with excess potassium bromide to produce 410 g of bromine

91%

for the reaction represented by the equation SO3 + H2O -> H2SO4, calculate the percentage yield if 500 g of sulfur trioxide react with excess water to produce 575 g of sulfuric acid

93.9%

what is the measured amount of product obtained from a chemical reaction

actual yield

What is the study of the mass relationships of elements in compounds?

composition stoichiometry

In most chemical reactions the amount of product obtained is

less than the theoretical yield

Which reactant controls the amount of product formed in a chemical reaction?

limiting reactant

The coefficients in a chemical equation represent the

relative numbers of moles of reactants and products

what is the maximum possible amount of product obtained in a chemical reaction

theoretical yield

for the reaction represented by the equation Pb(NO3)2 + 2KI --> PbI2 + 2KNO3 , how many moles of lead(II) iodide are produced from 300 g of potassium iodide and excess of PB(NO3)2

.904 mol

for the reaction represented by the equation C12 + 2KBr --> 2KCl + Br2 , how many moles of potassium chloride are produced from 119 g of potassium bromide

1.00 mol

(SA) How many grams of ammonium sulfate can be produced if 30 mol of H2SO4 react with excess NH3 according to the equation 2NH3(aq) --> (NH4)2SO4(aq)

3,960 g

for the reaction represented by the equation CH4 + 2O2 --> CO2 + 2H2O , how many moles of carbon dioxide are produced from the combustion of 100 g of methane

6.23 mol

A balanced chemical equation allows one to determine the

mole ratio of any two substances in the reaction

what is the ratio of the actual yield to the theoretical yield, multiplied by 100%

percentage yield