Definitions
This is what the process of determining the amounts of reactants and products in a chemical reaction is called.
What is stoichiometry?
Benzene, C6H6, is a known carcinogen that burns in the air according to the following equation:
2C6H6 + 15O2 --> 12CO2 + 6H2O
This is the mole ratio of O2 to C6H6.
What is 15:2?
When mercury(II) oxide, HgO, is heated, it decomposes to its elements, liquid mercury and oxygen gas:
2HgO --> 2Hg + O2
This is the molar mass of HgO.
What is 216.59 g/mol?
The following is a balanced equation for the combustion of butane with oxygen gas:
2C4H10 + 13O2 --> 8CO2 + 10H2O
Given the starting amount of 0.500 mol C4H10 and 3.50 mol O2, this is how many significant figures you should round your answer to.
What is 3 significant figures?
This is what the amount of product actually obtained in the laboratory from a chemical reaction is called.
What is actual yield?
Benzene, C6H6, is a known carcinogen that burns in the air according to the following equation:
2C6H6 + 15O2 --> 12CO2 + 6H2O
This is the amount of moles of O2 required to react with 1 mol of C6H6.
What is 7.5 mol O2?
When mercury(II) oxide, HgO, is heated, it decomposes to its elements, liquid mercury and oxygen gas:
2HgO --> 2Hg + O2
If 2.00 g HgO is decomposed, this is the amount amount (in moles) of HgO used.
What is 0.00923 mol HgO?
The following is a balanced equation for the combustion of butane with oxygen gas:
2C4H10 + 13O2 --> 8CO2 + 10H2O
Given the starting amount of 0.500 mol C4H10 and 3.50 mol O2, this is the limiting reactant.
What is C4H10?
This is what the reactant that is completely used up in the reaction and determines the amount of product that can form is called.
What is limiting reactant?
Benzene, C6H6, is a known carcinogen that burns in the air according to the following equation:
2C6H6 + 15O2 --> 12CO2 + 6H2O
This is the amount of moles of O2 required to react with 0.38 mol C6H6.
What is 2.9 mol O2?
When mercury(II) oxide, HgO, is heated, it decomposes to its elements, liquid mercury and oxygen gas:
2HgO --> 2Hg + O2
If 2.00 g HgO is decomposed, this is the amount amount (in moles) of Hg formed.
What is 0.00923 mol Hg?
The following is a balanced equation for the combustion of butane with oxygen gas:
2C4H10 + 13O2 --> 8CO2 + 10H2O
Given the starting amount of 0.500 mol C4H10 and 3.50 mol O2, this is how much the leftover reactant will be in excess.
What is 0.25 mol O2?
This is the maximum amount of product that can be obtained in a chemical reaction from known amounts of reactants, assuming all of the limiting reactant is consumed.
What is the theoretical yield?
Suppose you have a piece of aluminum that you want to react completely by the following single-displacement reaction:
2Al + 6HNO3 --> 2Al(NO3)3 + 3H2
This is the ratio used to convert from a known number of mol Al to the number of moles of HNO3 needed.
What is 2 mol Al:6 mol HNO3?
When mercury(II) oxide, HgO, is heated, it decomposes to its elements, liquid mercury and oxygen gas:
2HgO --> 2Hg + O2
If 2.00 g HgO is decomposed, this is the amount amount (in grams) of Hg formed.
What is 1.85 g Hg?
DOUBLE JEOPARDY!!!
The following is a balanced equation for the combustion of butane with oxygen gas:
2C4H10 + 13O2 --> 8CO2 + 10H2O
Given the starting amount of 0.500 mol C4H10 and 3.50 mol O2, this is how much CO2 will be made (in moles).
What is 2.00 mol CO2?
This is what the amount of product actually obtained expressed as a proportion to the amount expected is called.
What is percent yield?
Suppose you have a piece of aluminum that you want to react completely by the following single-displacement reaction:
2Al + 6HNO3 --> 2Al(NO3)3 + 3H2
If you added enough nitric acid so that all of the aluminum reacts, this is the mole ratio used to determine the moles of H2 produced.
What is 2 mol Al:3 mol H2?
When mercury(II) oxide, HgO, is heated, it decomposes to its elements, liquid mercury and oxygen gas:
2HgO --> 2Hg + O2
If 2.00 g HgO is decomposed, this is the amount amount (in grams) of O2 formed.
What is 0.148 g O2?
The following is a balanced equation for the combustion of butane with oxygen gas:
2C4H10 + 13O2 --> 8CO2 + 10H2O
Given the starting amount of 0.500 mol C4H10 and 3.50 mol O2, this is how much H2O will be made (in grams).
What is 45.1 g H2O?