name · web view1 egg (l) + 1 cup of flour (s) + 2 cups of chocolate chips (s) 8 chocolate chip...
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Name……………………………………………… Period………………Unit 7: Reactions and Stoichiometry…..Time to Over React
Skills: 1. Identify the when a reaction has
taken place based on chemical change
2. Use REP table to given balance reactions
3. Identify Single Replacement, Combustion and Decomposition Rxns
4. Complete SR reactions given reactants
5. Balance and ID Double replacement rxns
6. Predict unknown reactants and products
7. Calculate a mole ratio8. Use a mole ratio to calculate the
#of moles of reactants and products used in a rxn
Unit 7: Vocabulary: Complete throughout unit. Due on test day!
Word DefinitionReaction
Reactant
Product
Phase
Chemical Change
Yield
Precipitate
Balanced
Conservation of Mass
Combustion
Single Replacement
Double Replacement
Stoichiometry
Skill 1: Identify occurrence of a chemical reaction based on chemical change indicator
Chemical EquationsA chemical
equation
shows what takes place during a chemical reaction. Let’s break down the elements of a chemical equation… (hehehe)
Remember………Physical Change Chemical Change
It does NOT change ________________________,
it just changes
___________________________________
A change that does NOT affect a substance’s chemical composition
Changing ________________________________
into a ____________________________________
________________________________________
A color change may occur and a ________________________________________
_________________________________________Physical Change Phrases Chemical Change Phrases
1 egg (l) + 1 cup of flour (s) + 2 cups of chocolate chips (s) 8 chocolate chip pancakes (s)
Symbol/Vocabulary Explanation Pancake Model
The “Ingredients” of a chemical reaction!
The end result!
“Yields,” separates reactants from
products(s), (l), (g)
Designates an aqueous solution; the substance is dissolved in water.
Coefficient
Determine if a chemical reaction has taken place in the below situations: Breaking Glass ____________ Dissolving Sugar ___________ Rusting iron_________________ Boiling Water_______________
Digesting Sugar_____________ Burning Gasoline____________ Forming Ozone______________ Cooking Eggs_______________
Skill 2: Use REP or other Method to balance Chemical Equations
Problem: The above chemical reaction breaks the Law of Conservation of Mass:
Matter is neither ___________________ or ___________________ in a chemical reaction.
So… the ___________ of atoms must remain _______________ in a reaction
Balancing Equations : _________________________ are used to balance the number of at atoms of each element on both sides of the reaction. Coefficients must be the __________________whole number that balance the reaction.
Number and kind of elements on the left (Reactants) is equal to the number and kind on the right (Products)!
M&M Balancing:
1. With your M&Ms, create CH4 +O2.
2. USING THE SAME M&Ms, create CO2 +H2O.
3. Did you need any more M&Ms for the second group of elements? ____________________________________________________________________________________________________________________________________________________________________________
4. Could we describe this as a balanced reaction? 5. ______________________________________________________________________________________
______________________________________________________________________________________
6. Which are the reactants and which are the products? ____________________________________________________________________________________________________________________________________________________________________________
7. On your whiteboard, write out the balanced chemical reaction. Label the reactants, products and yield sign. Eat M&MS.
Challenge Balance: _______Na + ________ MgCl2 ______NaCl + ________Mg
Example: HCl (aq) + Zn (s) H2(g) + ZnCl2(aq) (NOT BALANCED)
NOTE: Coefficients can be changed, HOWEVER, subscripts CANNOT!
Draw:
Draw:
Using the REP Method:
Example: ____ HCl (aq) + ____ Zn (s) ____ H2(g) + ____ ZnCl2(aq)
Examples: Balance the following chemical reactions
1. _____ N2 + _____ H2 _____ NH3 2. _____ Al2O3 _____ Al + ____ O2
3. _____ Al + _____ Br2 ____ AlBr3 4. _____ AlBr3 + _____ Cl2 ____ AlCl3 + _____ Br2
5. _______Fe + ______O2 ______Fe2O3 6. _______H2 + ________O2 _______H2O
Reactants Elements
Products
H
Cl
Zn
ElementsElements
ElementsElements
ElementsElements
When a polyatomic ion is present AND it stays completely _______ during the reaction!
1. __Al + __CuSO4 ------> ___Al2(SO4)3 + ___Cu
2. ___Pb(C2H3O2)+ ____HCl → ____PbCl2 + ____H(C2H3O2)
If a polyatomic ion is present on one side of the equation and not on the other, you are forced to ________ it apart and balance each atom.
___SO3 (g) + ___ H2O ____H2SO4 (aq)
R E P
Al
Cu
SO4
R E P
Pb
H
Cl
(C2H3O2)
R E P
S
O
H
Name_______________________ Balancing Homework Period_____
Balance the equations below Using the REP method:1) ____ KClO3 ____ KCl + ____ O2
2) ____ NaCl + ____ F2 ____ NaF + ____ Cl2
3) ____ Pb(OH)2 + ____ HCl ____ HOH + ____ PbCl2
4) ____ AlBr3 + ____ K2SO4 ____ KBr + ____ Al2(SO4)3
5) ____ CH4 + ____ O2 ____ CO2 + ____ H2O
R E P1 x 2=2 K 1 x
2=21 x 2=2 Cl 1 x
2=23x2=6 O 2x3=6
6) ____ FeCl3 + ____ NaOH ____ Fe(OH)3 + ____NaCl
7) ____ P + ____O2 ____P2O5
8) ____ Na + ____ H2O ____ NaOH + ____H2
9) ____ Ag2O ____ Ag + ____O2
10) ____ S8 + ____O2 ____ SO3
Skill 3: Identify Synthesis, Single Replacement, Combustion and
Decomposition Rxns
Balancing: Balance the following reactions:
1. ____ S + ____ O2 ____ SO3 2. ____ P4 + ____ O2 ____ P2O3
3. ____ C + ____ H2 ____ C3H8 4. ____ CaO + _____H2O _____ Ca(OH)2
Real World Example: Magnesium and Oxygen combine to from Magnesium Oxide!
____ Mg (s) + ____ O2 (g) ____ MgO (s)
Balancing: Balance the following synthesis reactions:
1. ____ HgO ____ Hg + ____ O2 2. ____ Al2O3 ____ Al + ____ O2
3.____ AgCl ____ Ag + _____ Cl2 4. ____ H2O2 (l) ____ H2O (l) + ______ O2 (g)
Synthesis: When two or more reactants combine to form ____ ________________ product
General Equation: ________________________________
Decomposition: A ______________________ compound is _________________ down (________________) into ____________ or _______________ ____________________ substances
General Equation: ________________________________
Elements
Elements
Elements
Elements
Real World Example: Hydrogen peroxide decomposes into water and oxygen!
Balancing: Balance the following reactions:
1. ___C4H12 + ____ O2 ____ H2O + ______ CO2 2. _______C2 H6 + _____ O2 ______ H2O + _______ CO2
Skill 4: Complete SR reactions given reactants
Balancing: __Zn + __HCl __ZnCl2 + __ H2 ____ Li + ___ HOH ____ LiOH + ___H2
Finish the Chemical Reaction:Use Table J to see if the following reactions can occur. If it can, write the product and balance the equation (if necessary).
1. ____ Zn + ____ H2SO4 ___________________________
2. ____Pb + _____ FeCl3 ___________________________
3. ____ Cl2 + _____ LiI ____________________________
Combustion: An __________________ compound (contains ____ and ____) reacts with ______________ and creates ONLY _______________________ and ________________________
General Equation: ________________________________
Single Replacement Reactions: For a single replacement reaction to occur, the lone metal listed must be ________ on Reference Table J than the metal in the compound in order for it to “________________” the metal in the compound.
General Equation:
Elements
Name_______________________________ Period___________
Balance each and determine the type of reaction. (Synthesis, Decomposition, Combustion, SR)
TYPE:
1.) ____CaO + ____P2O5 ____Ca3(PO4)2 ________________
2.) ____ Ag + ____ H2S ____ Ag2S + ____ H2(s) ________________
3.) ____ N2O5 ____ N2 +____ O2 ________________
4.) ____ C3H8(g) + ____ O2(g) ____ CO2(g) + ____ H2O(g) ________________
5.) ____ NaClO3(aq) ____ NaCl(aq) +____ O2(g) ________________
Name _______________________Bell Ringer Single Replacement PracticeFor each of the following determine whether or not a single replacement reaction will occur using Reference Table J. If it does write out products and balance the reaction.
1. ____Ca + ____H2O
2. ____Zn + ____HCl
3. ___Ag + ___AuCl3 → ___AgCl + ___Au
4. ____Cr + ___H2SO4 → ___Cr2(SO4)3 + ___H2
5. ____Cr + ____FeCO3 → ___Cr2(CO3)3 + ____Fe
Name _______________________Bell Ringer Single Replacement PracticeFor each of the following determine whether or not a single replacement reaction will occur using Reference Table J. If it does write out products and balance the reaction.
1. ____Ca + ____H2O
2. ____Zn + ____HCl
3. ___Ag + ___AuCl3 → ___AgCl + ___Au
4. ____Cr + ___H2SO4 → ___Cr2(SO4)3 + ___H2
5. ____Cr + ____FeCO3 → ___Cr2(CO3)3 + ____Fe
Name _______________ Date________ Period____ Single Replacement Reactions
Background Information:
The tendency of a particular element to combine with other substances is a measure of the ACTIVITY of that element. The more active an element is, the more likely it is to combine. In a single replacement reaction, an uncombined element replaces a less active element in a chemical compound, leaving the less active element as a single product!
Purpose: In this investigation, you will observe how various metals undergo single replacement reactions when placed in acid.
Problem: How does a single replacement reaction occur?
Materials: (per group)
Safety goggles, 5 test tubes1M hydrochloric acid test-tube rackGraduated cylinder ZincCopper (cut wire in to pieces of 1-cm length) AluminumIron (nail) Magnesium (cut into 1-cm lengths)
Procedure:
1. Label your test tubes with the names of the metals listed in the materials.
2. Put on your safety goggles. Carefully pour approximately 5 mL of HCl into each test tube. (Make sure the amount of HCl is the same in each test tube.
3. One, at a time, place the appropriate metal in each test tube. Record your observations for each metal. Feel each test tube as the reaction proceeds and record your observations.
4. When you have completed the investigation, carefully pour off the acid, rinse the metal several times with water, and put it into a container provided by your teacher. Do not put any unused metal in the sink.
Zinc + copper sulfate zinc sulfate + copperZinc replaces the less active copper, combines with sulfate, and frees the copper from the
compound.
Observations:
Conclusions:
1. Were these reactions endothermic or exothermic? _________________ Explain_________________________________________________________________________________________________________________________________________
Critical Thinking and Application
1. Which of the metals are more active than hydrogen?_________________
2. Which of the metals are less active than hydrogen?_____________________
Metal Reacted with
HCl
Observations: Balanced Single Reaction Equation
Magnesium (Mg)
Aluminum (Al)
Iron (Fe)
Copper (Cu)
Zinc (Zn)
3. The rate at which hydrogen gas is produced is a result of these single replacement reactions is an indication of the relative activity of the metals. List the order of their activity from most active to least active. _________________________________________________________
Skill 5: Balance and ID Double replacement rxns
Bottom Line: Double replacement is a double flip-flop!
Balancing: Balance the following reactions:
2. ____ BaCl2 ( )+ ____ H2SO4 ( ) ____ BaSO4 ( )+ _____ HCl ( )
3. ____ Al(NO3)3 ( ) + ____ NaOH ( ) ____ Al(OH)3 ( )+ _____ NaNO3 ( )
4. ____ Ca(OH)2 ( ) + ____ H2SO4 ( ) ____ HOH ( )+ ____ CaSO4 ( )
Double Replacement :Involves an exchange of positive ions between two reacting ______________ _________________
Reaction will only occur if a ___________, _____________, or __________ is formed
Precipitates: _______________________________________________________________________
See Table ___________
Examples: CuNO3 _____ PbCl2 ______ Ca3(PO4)2 ______ Ba(OH)2 _______
General Equation: ________________________________
Step-by-Step Problem Solving: 1. Write products by switching element/polyatomic of the
reactants 2. Check solubility on Table F.
Soluble --> (aq)Insoluble--> (s)= precipitate = means a reaction occurs
Elements
Double Replacement Practice:
____ K2CO3 (aq) + ____ BaCl2 (aq) ____ KCl (aq) + ____ BaCO3 (s)
KCO3BaCl
Part 1 – Finish and Balance the Reaction: Remember to criss-cross.
1. ___ AgNO3 (aq) + ____ K3PO4 (aq) _______________________________________
2. ___ Ca(C2H3O2)2 (aq) + _____ Na2CO3 (aq) _________________________________
3. ___ BaCl2 (aq)+ ___ Na3PO4 (aq) ________________________________________
4. ___ Na2S (aq) + ____ MgCl2 (aq)__________________________________________
Part 2 – Chemical Reactions in Words: Remember to criss-cross.
1. Silver Nitrate reacts with magnesium chloride
2. Iron (III) chloride reacts with sodium hydroxide
3. Sodium phosphate reacts with calcium hydroxide
Name________________________________Period____
Double Replacement ReactionsIntroduction: A double displacement reaction or metathesis reaction involves the reaction of two compounds to form two new compounds. In effect, the compounds change partners with each other. This experiment will provide you with opportunities to observe several of these double displacement reactions. Purpose:
To observe the formation of new substances in double displacement reactions. To write and balance chemical equations for double replacement reactions
Procedure: 1. Combine the 2 solutions as indicated on your chart in a well of the tray.
2. Make observations about the reaction that you see
3. Repeat procedure for the remaining pairs of chemicals
4. Clean the tray and dispose of the wastes in the waste container provided.
Questions:1. What evidence is there that a chemical change occurred?
2. How you might be able to determine which of the products is the precipitate._________________________________________________________________________________________________________________________________________________________
3. Which reaction did not produce a visible reaction? __________ with __________
4. Write out the reaction of this combination:
5. Are the products soluble or insoluble according to Table F?___________________
Finish the Chemical Reaction:Write the products and balance the equation (if necessary). Remember to criss-cross and pay attention to diatomic elements (BRINCLHOF)
1. ____ Na2S ( ) + _____ Cd(NO3)2 ( ) _____________________________
Reactant #1 Reactant #2 EVIDENCE OF CHEMICAL CHANGE (Observations)
1 NaCl (aq) Ag(NO3) (aq)
2 NaOH (aq) Fe2(SO4)3 (aq)
3 NH4OH (aq) K2CO3 (aq)
4 Pb(NO3)2 (aq) KI (aq)
5 NaOH (aq) Cu(NO3)2 (aq)
6 Ag(NO3) (aq) KI (aq)
2. ____BaCl2 ( ) + H2SO4 ( ) _____________________________________
3. ____ BaCl2 ( ) + _____ K2CO3 ( ) _________________________________
Skill 6: Predict unknown reactants and products
When determining the missing reactants or products, you must always remember:
1) The Law of Conservation of Matter 2) Balance!!3) That BrINClHOF’s come in pairs (Remember 7-Up!)4) Always criss-cross when forming new compounds!
1. _ N2+ ___ H2 ___ NH3 Type: ____________
2. ___ K + ___ Mg(NO3)2 Type: ____________
3. ___ Na3(PO4)(aq) + ____ Ca(OH)2 (aq) Type: __Double R.__
General Equations Synthesis : A + B AB Decomposition : AB A + B Single Replacement : A + BX B +
AX Double Replacement :
AX (aq) + BY(aq) AY + BX Combustion :
Organic Compound + O2 CO2 + H2O
Example:H2 + Cl2 ___________ Type: _________
O2 + Fe __________ Type: _________
4. ____ F2 + ___ AlCl3 Type: ____________
5. ____ C2H6 + ____ O2 Type: ____________
6. ____ HCl (aq) + _____ Mg(OH)2 (aq) T ype: ____Double R.__
7. ____ Ba(s) + ____ K2(CO3) Type: ____________
8. _____ Ag2O Type: ____________
9. _____ H2(SO4)(aq) + ____ Na(OH)(aq) Type: __Double R.__
10.____ Zn(s) + _____ MgBr2(aq) Type: ____________
11. ____H2 + ____ O2 Type: ____________
Matching Reaction Types & Products
Reaction Type Reactants yield Products
C3H8 + O2
Zn + HClDouble Replacement KI + Pb(NO3)2
Mg(ClO3)2
Al2O3
F2 + KBr
Na + Cl2Reaction Type Reactants yield Products
C6H12 + O2
K2CO3
MgCl2 O2 AlO2 K2O CO2
CO2 H2O NaClCO H2O ZnCl2H2 KNO3 PbI2KF Br2
Synthesis Decomposition Combustion
Single Replacement Double Replacement Synthesis
Synthesis Decomposition Combustion
Single Replacement Double Replacement Synthesis
The Hamburger Analogy
Based on this recipe:
1. If I have five double cheeseburgers:
a. How many hamburger buns do I have?____________
b. How many hamburger patties do I have?___________
c. How many slices of cheese do I have?_____________
d. How many strips of bacon do I have?______________
2. How many bacon double cheeseburgers can you make if you start with:
a. 1 bun, 2 patties, 2 slices of cheese, 4 strips of bacon.
b. 2 buns, 4 patties, 4 slices of cheese, 8 strips of bacon.
c. 1 dozen buns, 2 dozen patties, 2 dozen slices of cheese, 4 dozen strips of bacon.
d. 1 mole bun, 2 mole patties, 2 mole slices of cheese, 4 mole strips of bacon.
e. 10 buns, 20 patties, 20 slices of cheese, 40 strips of bacon.
3. If you had fixings for 100 bacon double cheeseburgers, but when you were cooking you ruined 10 of them. What percentage of the bacon double cheeseburgers do you actually make?
Miss Hull’s recipe for a bacon double cheeseburger:1 hamburger bun
2 crabby patty hamburger patties 2 slices of cheese 4 strips of bacon
Here are two examples of chemical recipes:
2 Na + Cl2 2 NaCl
1 mole of H2SO4 + 2 mole of NaOH 1 mole Na2SO4 +2 mole H2O
Based on the RECIPES above:
1. If I have 2 moles of NaCla. How many moles of sodium do I have?
b. How many moles of Chloride do I have?
2. If I want to make 5 moles of Na2SO4:a. How many moles of H2SO4 do I need?
b. How many moles of NaOH do I need?
3. How much Na2SO4 can I make if I have:a. 1 mole of H2SO4 and 2 mole of NaOH
b. 10 mole of H2SO4 and 20 mole of NaOH
c. 0.1 mole of H2SO4 and 0.2 mole of NaOH
d. 1 mole of H2SO4 and 20 moles of NaOH
e. 0.42 mole of H2SO4 and 0.65 mole of NaOH
f. 5 grams of H2SO4 and 5 grams of NaOH
Skill 7: Calculate a mole ratio: Flipped Lesson!
Now, the Chemistry Part!The math and the concepts are identical as the other example. The only
difference is the recipe.
Stoichiometry: This is the word for that part of chemistry that involves the mass and volume relationships in chemical changes.
Example 1: _____ H2 + ____ O2 ____ H2O
How many moles of each of the substances? ____ H2 ____ O2 ____ H2O
What is the mole ratio of O2 to H2?
If I want to burn 5 moles of O2, how many moles of H2 gas is needed?
MolesUnknown=Knownmoles× unknowncoefficientknowncoefficient
Example 2: How many moles of ammonia (NH3) are produced when 0.60 mole of nitrogen reacts with hydrogen? (first balance)
_____ N2 + ____ H2 ____ NH3
Example 3: How many moles of aluminum are needed to form 3.7 mol of Al2O3? (first balance)
_____ Al (s) + ____ O2 (g) ____ Al2O3 (s)
SKILL #7: MOLE TO MOLE problems
Four Steps:
1. Write the balanced equation. The equation must be balanced correctly or the ratio between reactants and products will not be correct.
2. Find the number of moles of the given substance.
3. Inspect the balanced equation to determine the ratio of moles of required substance to moles of given substance.
…. Moles of required substance … (stoichiometry part) Moles of given substance
4. Express the moles of required substance into what unit is needed to finish the problem.
1. Given the balanced equation: 2 H2 + O2 2 H2OHow much water will be producedif 5 moles of H2 is completely reacted?
2. Given the balanced equation: 2 H2 + O2 2 H2OHow much oxygen will be consumedif 5 moles of H2 is completely reacted?
3. Given the balanced equation: 4 NH3 + ____O2 ___ NO + 6 H2O
If 12 moles of O2 are consumed, how Many moles of NO are produced?
4. Given the balanced equation: __NH3 + ___O2 ___ NO + ____ H2O
If 3 moles of O2 are completely consumed, how Many moles of NH3 are consumed?
Calculate the number of moles in each problem. Use highlighted quantities.
a. Ca + 2H2O Ca(OH)2 + H2 1 = 2 X 6 X = 3 mol Ca
b. 2N2O5 4NO2 + O2
c. 2Li+ H2SO4 Li2SO4 + H2
Name ________________________________Date ___________________
S’more Stoichiometry
d. 3H2 + N2 2NH3
e. 2C2H2 + 5O2 4CO2 + 2H2O
f. CH4 + 2O2 CO2 + 2H2O
Definitions: ‘Stoichio’ means element and ‘metry’ means the process of measuring. The mass and quantity relationships among reactants and products in a reaction are found using the process of stoichiometry.
Problem:1) How many boxes of graham crackers, bags of marshmallows and chocolate bars
are needed to make enough S’mores for everyone in class?
Solutions:1.) Write a balanced chemical equation using the following symbols from the data table below:
What is the G.F.M. of a S’More? _________________
What do the coefficients represent? _______________________________________________________
2.) a. Determine how many graham crackers are needed to make 17 S’mores (17 people in this class).
b. Determine how many chocolate squares are needed to make 17 S’mores (17 people in this class). .
3.) a) How many total marshmallows are needed for this lab? ________
b) Determine the mass of all the marshmallows needed for this lab.
c) How many bags of marshmallows are needed for this class? _______________
4.) Determine the total mass of graham crackers and chocolate segments needed for this lab:
a) Graham Crackers b) Chocolate Segments
5.) a. In this case, if a box of graham crackers has a mass of 408 g, how many boxes do you need?
____Gr2MCh4
Substance Symbol Unit Mass BoxGraham Cracker Gr 7.43 grams 408.0 gMarshmallow M 8.84 grams 283.0 gChocolate Pieces
Ch 3.76 grams 111.0 g
S’more Gr2MCh4
b. If one chocolate bar has a mass of 15.04 g, how many bars do I need?
6.) If I bought 1 box of graham crackers, 20 bars of chocolate and 1 bag of marshmallows, which part of the S’more recipe is going to be the limiting reactant? ___________________________ (Which part of the recipe will limit how many S’more you can make?)
Additional Questions: Re-write your balanced S’mores equation: ____________________________________________
7.) a. Based on your balanced equation, how many S’mores can you make if you have 75 marshmallows?
b. Based on your balanced equation, how many S’mores can you make if you have 75 piece of chocolate?
8.) a. If you want to make 10 S’Mores how many graham crackers will you need?
b. How many chocolate pieces will you need?
9.) Using a wooden skewer, CAREFULLY toast your marshmallow over a Bunsen Burner using a blue flame and make your S’more!!
Name___________________ Stoichiometry Practice: Period_____
Directions: Solve the following stoichiometry problems. Assume all gases are at STP. Don’t forget to write out your balanced chemical equation. Make sure to show ALL work to receive FULL CREDIT!
1.Calculate the number of moles of oxygen required to react completely
2. Calculate the moles of oxygen produced from the decomposition of
with 14.8 mol Al in the following equation:
___Al(s) + ____O2(g) _____Al2O3(s)
= 11.1 mol O2
0.61 moles of potassium chlorate (KClO3).
_____KClO3 ______KCl + ______O2
3. If 20.0g grams of zinc react with excess hydrochloric acid, how many grams of zinc chloride (ZnCl2) are produced?
___Zn(s) + _____HCl(aq) ____ZnCl2(aq) + _____H2(g)
4. How many grams of chlorine gas must be reacted with excess sodium iodide (NaI) if 10.0 grams of sodium chloride (NaCl) are needed
_______NaI(aq) + __Cl2(g) _____NaCl(aq) + _____I2(g)
5. How many grams of copper are required to replace 4.00 grams of silver nitrate which are dissolved in water?__Cu(s)+ ____AgNO3(aq) ___Cu(NO3)2(aq) +__Ag(s)
6. How many moles of hydrogen gas are needed to react with 15.1 g chlorine gas to produce hydrogen chloride gas?
___H2(g) + __Cl2(g) _____HCl(g)
14.8 moles Al
3 moles of O24 mole Al
All You Need Is Stoich PUT THIS INTO THE ROCKET SOCRATIVE THING
1. Balance the following reaction:
_____C2H4 (g) + _____O2 (g) _____CO2 (g) + _____H2O(l)
Give the following mole ratios:
a. C2H4 to O2 _______________
b. CO2 to H2O __________
c. H2O to O2________________
d. H2O to C2H4 ______________
What type of reaction is this?If you start with 1.50 moles of C2H4 , how many moles of O2 do we need to react with it?
If you start with 1.50 moles of C2H4 , how many moles of CO2 are formed?
2. Balance the following reaction:
_____ Fe(s) + _____ Cl2 (g) _____ FeCl3 (s)
If you have 0.600 moles of Cl2 , how many moles of iron do you need to completely react with it?
If you react 0.600 moles of chlorine gas, how many moles of FeCl3 would you produce?
1. Balance the following reaction:
_____ P4 (s) + _____ O2 (g) _____ P4O10 (s)
If 2.500 moles of P4 are available for this reaction, how many moles of O2 (g) are necessary to react all of it?
How many grams of P4O10 would you produce in this reaction?
2. For the reaction: 4Li (s) + O2 (g) 2 LiO (s)calculate the mass in grams of lithium oxide formed from 0.283 mole of lithium.
3. For the reaction: N2 (g) + O2 (g) 2NO (g)calculate the number of grams of NO that are produced from 2.00 mol moles of oxygen gas.
4. Given: 2H2 (g) + O2 (g) 2 H2O (l)Find the number of grams of hydrogen gas that will react with 2.50 moles of oxygen gas.
5. Given: 2 K (s) + Br2 (g) 2 KBr (s)How many grams of KBr can be formed from 40.0 g of bromine gas?
6. Given: Cu (s) + 2AgNO3 (aq) 2Ag (s) + Cu(NO3)2 (aq)
a. How many grams of copper (II) nitrate can be formed from 0.25 moles of silver nitrate?
b. Calculate the number of grams of Cu needed to react with 10.8 grams of AgNO3 ?
7. When heated, potassium chlorate decomposes to potassium chloride and oxygen gas. Write a balance reaction for the decomposition of potassium chlorate.
8. How many grams of each product will be produced by the decomposition of 1.00 grams of potassium chlorate?