Based on the following chemical equation 2C6H6+ 15O2–> 12CO2 + 6H2O calculate the number of moles of CO2 that will be produced when 8.90 moles of H2O are produced as well?
How many moles of molecular oxygen will be needed for the complete combustion of 100.0 g of sulfur dioxide? The product of this reaction is sulfur trioxide.
How many grams of molecular chlorine will be required to completely react with 0.0223 moles of sodium iodide according to the following reaction: 2NaI + Cl2 –> 2NaCl + I2
How many molecules of O2 will be required to react completely with 0.600 moles of H2 in order to form water?
How many grams of O2 are required to produce 1.23 x1024
molecules of water? 2H2+ O2 –> 2H2O
Calculate the number of moles of excess reactant that will be left-over when 56.0 g of CaCl2 react with 64.0 g of Na2SO4
: CaCl2+ Na2SO4–>CaSO4+ 2NaCl
How many moles of HF will be produced by the complete reaction of 1.42moles of H2 in the following equation? H2+ F2–> 2HF
How many moles of N2 will be consumed when 1.60 moles of H react completely in the following equation? N2+ 3H2 –> 2NH3
How many moles of CO2 are produced when 3.01 x 10
23 molecules of C3H6 react completely in the following equation? 2C3H6+ 9O2 –> 6CO2+6H2O
How many molecules of NH3 are produced when 3.00 moles of H react completely in the following equation? N2+ 3H2
What mass of HCl is produced when 3.00 moles of H2 react completely in the following equation? H2+ Cl2 –> 2HCl
What mass of carbon monoxide is produced when 1.50 moles of oxygen react completely in the following equation? 2C + O
How many moles of N2O5 are produced when 3.00g of O2
react completely in the following equation? 2N2+ 5O2–> 2N2O5
What mass of oxygen is consumed when 54.0g of water is produced in the following equation? 2H2+ O2 –> 2H2O
What mass of CO2 is produced when 50.0g of C2 H
reacts completely in the following equation? C2H4 + 3O2–> 2CO2 + 2H2O
Which is the limiting reactant when 12.0 moles of CH
are reacted with 20.0 moles of O2 in the following equation? CH4 + 2O2 –> CO2 + 2H2O
Which substance is in excess when 6.00 moles of aluminum are reacted with 12.00 moles of oxygen in the following equation? 4Al + 3O2 –>2Al2O3
In a reaction to produce sulfuric acid, the theoretical yield is 300.g. What is the percent yield if the actual yield is 280.g?
What is the percent yield for a reaction in which 342g of a product is actually produced when the theoretical yield is 400.g?
Calculate the percent yield for the following reaction if 233 g of NO reacted and 175 g of HNO3 were produced. 3NO2 + H2O –> 2HNO3+NO