CHEM 1A03 Lecture Notes - Lecture 6: Chemical Equation, Stoichiometry, Silver Nitrate

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28 Jun 2016

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Stoichiometry and Quantities in Chemical Reactions

 applying the relationships between the molar quantities of reactants and products involved in

chemical reactions to perform calculations

 the mole ratio is the ratio of the amount in moles of reactants and/or products in a chemical

reaction that arises from the coefficients in a balanced chemical equation

2 H2O  2 H2 + 1 O2

2 mol of water : 2 mol of hydrogen : 1 mol of oxygen

2

OHofmoles

Hofmoles

For every 2 moles of water decomposed, 2 moles of hydrogen gas is made.

OHofmolesHofmoles 22 2

2

The moles of hydrogen will equal the moles of water reacted.

 If 10.0 mL of water is decomposed,

Mass of water reacted

  

   



  

Moles of water reacted

 



 



  

Moles of hydrogen produced

 

 

  

0.555 mol of hydrogen will be produced.

2

OHofmoles

Oofmoles

For every 2 moles of water decomposed, 1 mole of oxygen gas is made.

OHofmolesOofmoles 22 2

1

The moles of oxygen will be half the moles of water reacted.

 If 10.0 mL of water is decomposed,

Mass of water reacted

  

   



  

Moles of water reacted

 



 



  

Moles of oxygen produced

 

 

  

0.277 mol of oxygen will be produced.

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CHEM 1A03 Full Course Notes

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Document Summary

For every 2 moles of water decomposed, 2 moles of hydrogen gas is made. moles. The moles of hydrogen will equal the moles of water reacted. 0. 555 mol of hydrogen will be produced. moles. For every 2 moles of water decomposed, 1 mole of oxygen gas is made. moles. The moles of oxygen will be half the moles of water reacted. If 10. 0 ml of water is decomposed, In a chemical reaction, the amount of one substance must be known. Using the mole ratio, we can determine how much reactant is needed (or product will be made) 1 cu(s) + 2 agno3(aq) 1 cu(no3)2(aq) + 2 ag(s) For 1 mole of copper, 2 moles of silver nitrate is required. For 1 mole of copper, 2 moles of silver will be produced. Predict the mass of silver metal that will be produced. Excess reagent is the reactant that is present in more than the required amount to complete the reaction.

Related Questions

In the following chemical reaction, how many moles of O2 are needed to produce 2.8 mol of CO2? C2H6 + O2 â CO2 + H2O?

How many moles of methane are produced when 36.6 moles of carbon dioxide gas react with excess hydrogen gas?

How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 53.6 moles of water vapor?

Plants convert carbon dioxide and water to glucose (C6H12O6) and oxygen in the process of photosynthesis.

1.Write a balanced equation for this reaction.

2. Determine how many moles of CO2 are required to produce 42.0 mol of glucose.

How many grams of sulfur can be made in the following reaction if 17.0 grams of H2S reacted with excess SO2?

2 H2S + SO2 â 2 H2O + 3 S

The balanced chemical equation for the combustion of hydrogen and oxygen to give water is 2 H₂ + O_{2 -->} 2 H₂O

4) Complete the following sentence to describe the number of moles of each reactant involved in the combustion of hydrogen:

___ moles of hydrogen react with ___ moles of oxygen to give moles of water

When the reactants in a mixture are present in the exact mole ratio given by the balanced chemical equation, all of the reactants should be used up when the reaction is over. There will be no âleftoverâ reactants. However, if one of the reactants is present in an amount greater than its mole ratio, then that reactant cannot react completely, and some of it will be left over at the end of the reaction.

Use the mole ratio of hydrogen to oxygen from question 4 to determine what happens when various hydrogen/oxygen gas mixtures are allowed to burn. Complete the following table to indicate which reactant (H₂ or O₂) is present in excess, and how much of it will be left over after the combustion reaction is complete. Note: The second one has been completed as an example.

Parts H₂	6	5	4	3	2	1	0
Parts O₂	0	1	2	3	4	5	6
Which reactant is present in excess?	H2	H₂	None		O2		O2
How much of that reactant is left over?	6	3	N/A		3		6

Also, why does oxygen not immediately react with hydrogen during combustion?

Part A

Determine the balanced chemical equation for this reaction.

C8H18(g)+O2(g)?CO2(g)+H2O(g)

Enter the coefficients for each compound in order, separated by commas. For example, 1,2,3,4 would indicate one mole of C8H18, two moles of O2, three moles of CO2, and four moles of H2O.

2,25,16,18

Balanced chemical equation

2C8H18(g)+25O2(g)?16CO2(g)+18H2O(g)

Part B

0.240 mol of octane is allowed to react with 0.610 mol of oxygen. Which is the limiting reactant?


	oxygen

Part C

How many moles of water are produced in this reaction?

Express your answer with the appropriate units.

H2O produced =

Part D

After the reaction, how much octane is left?

Express your answer with the appropriate units.

CHEM 1A03 Lecture Notes - Lecture 6: Chemical Equation, Stoichiometry, Silver Nitrate

CHEM 1A03 Full Course Notes

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