How many moles of water are made by

Slides:

Advertisements

Similar presentations

Mass to Mass Stoichiometry

Advertisements

Chemical Quantities Chapter 9

Stoichiometry, Limiting Reactants and Percent Yield

Limiting Reactants Very rare that reactants are present in the same ratio that they are used in the rxn. This means one reactant will run out first. This.

Percent Yield and Limiting Reactants

Chemistry Notes Empirical & Molecular Formulas. Empirical Formula The empirical formula gives you the lowest, whole number ratio of elements in the compound.

Finding Theoretical Yield and Percent Yield

Mass Conservation in Chemical Reactions Mass and atoms are conserved in every chemical reaction. Molecules, formula units, moles and volumes are not always.

Notes #14, Ch. 9 Stoichiometry and Theoretical Yield.

Afra Khanani Period 6 Honors Chemistry March 31 st.

Things you must KNOW and what to expect  Things you must KNOW  You must KNOW your polyatomics  You must KNOW how to write a balanced formula  You have.

April 7, 2014 Today: Stoichiometry and % Yield. Percent Yield Remember, stoichiometry is used to tell you how much product you can form from X amount.

Afra Khanani Honors Chemistry Period 6 March 31 st.

STAAR Ladder to Success Rung 8. How do chemists define a mole? Example #1: A sample consists of 6.85 x atoms of carbon. How many moles does the.

Using the MOLE. Percentage composition Percentage composition is the mass of individual elements in a compound expressed as a percentage of the mass of.

 Mass of crucible + lid = g  Mass of crucible + lid + Mg = g  Mass of crucible + lid + magnesium oxide = g.

$100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300.

Moles of Compounds. A properly written compound shows the ratio of atoms in the compound. For example, sodium carbonate (Na 2 CO 3 ) shows that for every.

Take your periodic table out. What is atomic mass of Carbon Point where you can find it in the periodic table! 6 is atomic number not atomic mass Atomic.

Stoichiometry: A calculation based on a balanced equation. Granada Hills Charter High School.

Afra Khanani Period 6 Honors Chemistry March 31 st.

Stoichiometry Warmup I have 1 mole of CO 2 gas at STP. How many grams of CO 2 do I have? How many Liters of CO 2 do I have? How many molecules of CO 2.

PERCENT YIELD. Percent Yield Percent yield is the ratio of actual yield of an experiment to theoretical yield. To find percent yield, you divide the actual.

Products Percent Yield. Theoretical Yield Maximum amount of product Calculation Balanced Equation Given mass Molar Mass Mole Ratios.

Stoichiometry. Warm-Up Example of stoich problem Magnesium metal burns in the air Mg (s) + O 2(g) MgO (s) 2 Mg (s) + O 2(g) 2 MgO (s) 3g? g.

Follow the powerpoint as an example of how to calculate the mass of the barium phosphate product ( in filter paper)with your data, we will use only the.

Calculating Empirical Formulas

Chapter 9 Stoichiometry Test REVIEW SHEET

Ch. 9-3 Limiting Reactants & Percent Yield. POINT > Define limiting reactant POINT > Identify which reactant is limiting in a reaction POINT > Define.

Challenge Problem When nitrogen and hydrogen react, they form ammonia gas, which has the formula NH 3. If 56.0 g of nitrogen are used up in the reaction,

Mass-Mass Conversions 56.0 g N 2 x g N 2 g NH = 1904 = When nitrogen and hydrogen react, they form ammonia gas, which has the formula.

Actual Yield The amount of product formed from the actual chemical reaction and it is usually less than the theoretical yield.

Take your periodic table out. What is atomic mass of Carbon Point where you can find it in the periodic table! 6 is atomic number not atomic mass Atomic.

Stoichiometry. Stoichiometry Stoichiometry – the process of using a balanced chemical equation to calculate the relative amounts of reactants and products.

Honors Stoichiometry Examples. Example 1 What mass of carbon dioxide in grams is needed to react with 3.00mol of H 2 O in the following photosynthetic.

Chapter 9 Chemical Quantities in Reactions

Stoichiometry Mole-to-Mole:

Percentages of carbon, hydrogen and oxygen from combustion

Mathematics in Chemistry

Clicker #1 How many cars can we make? A) 3 B) 4 C) 6 D) 12 E) 16.

Clicker #1 How many cars can we make? A) 3 B) 4 C) 6 D) 12 E) 16.

Chapter 12 Review.

Chapter 12 Review.

What percent is 8 of 20? If a reaction made 50. g of product, but was supposed to produce 75. g, what was the percent produced? 8 20 x 100 = 40% 50.

Bell Ringer Jan. 31 N2 + 3H2  2NH3 How many moles of NH3 are created from 18 grams of H2? How many moles of N2 are needed to create 42.

Clicker #1 How many cars can we make? A) 3 B) 4 C) 6 D) 12 E) 16.

Quantity Relationships in Chemical Reactions

Molar Conversions (p.80-85, )

Combustion Analysis The composition of a substance is often determined by using a specified reaction to break down the substance into known measurable.

9.4 – NOTES Avogadro and Density

Gas Law Stoichiometry.

) ( ) ( ( ) ( ) ( ) ( ) 3.96 FIND CARBON FROM CO AND CO2

( ) ( ) ( ) = 2 C6H14(g) + 19 O2 (g) 12 CO2(g) + 14 H20(g) KNOWN

Unit 3 – Chemistry in Society Pupil Notes

( ) ( ) ( ) = 2 C6H14(g) + 19 O2 (g) 12 CO2(g) + 14 H20(g) KNOWN

Molecular Formula number and type of atoms covalent compounds

Clicker #1 How many cars can we make? A) 3 B) 4 C) 6 D) 12 E) 16.

Stoichiometry Problems

Bell Work: Limiting Reactant Problems

STOICHIOMETRY REVIEW.

Percent Yield Unit 7 Lesson 3.

Clicker #1 How many cars can we make? A) 3 B) 4 C) 6 D) 12 E) 16.

Clicker #1 How many cars can we make? A) 3 B) 4 C) 6 D) 12 E) 16.

The mole ratio.

Combustion analysis Combustion analysis is a method used in both organic chemistry and analytical chemistry to determine the elemental composition (more.

Mass to Mass Conversions

Presentation transcript:

How many moles of water are made by 2 C6H6 + 15 O2 → 12 CO2 + 6 H2O How many moles of water are made by burning 0.35 moles of C6H6? 6 mol H2O = 3 = X 2 mol C6H6 1 0.35 X = 1.1 mol H2O

What is the mole ratio between the products? Label with the formulas. 2 C6H6 + 15 O2 → 12 CO2 + 6 H2O What is the mole ratio between the products? Label with the formulas. 12 CO2 = 2 CO2 6 H2O = 1 H2O 6 H2O 1 H2O or 12 CO2 2 CO2

How many grams of carbon dioxide are 2 C6H6 + 15 O2 → 12 CO2 + 6 H2O How many grams of carbon dioxide are made by burning 18.0 g of C6H6? 2 C6H6 = 1 C6H6 = 78.0 g C6H6 = 18.0 g 12 CO2 6 CO2 264 g CO2 X X = 60.9 g CO2

2 C6H6 + 15 O2 → 12 CO2 + 6 H2O If the actual lab result from burning 18.0g C6H6 is 45.6 grams CO2, how much is the % yield? % yield = Actual (lab) result x 100 % Theoretical (calculated) % yield = 45.6 g x 100 = 74.9 % 60.9 g

2 C6H6 + 15 O2 → 12 CO2 + 6 H2O How many grams of water are made by burning 78.0 g of C6H6 with 220.0 g of oxygen? 2 mol C6H6 = 156 g C6H6 = 78.0 g 6 mol H2O 108 g H2O X X = 54.0 g H2O 15 mol O2 = 480 g O2 = 220.0 g O2 6 mole H2O 108 g H2O X X = 49.5 g H2O