Cheat Sheet for Chemical Equilibrium
... • All ICE charts you see on the AP exam follow the 5% rule. That means when you subtract “x” or add “x” from a concentration other than 0, you can ignore it! ...
... • All ICE charts you see on the AP exam follow the 5% rule. That means when you subtract “x” or add “x” from a concentration other than 0, you can ignore it! ...
Chapter 4 Packet
... molecular and net ionic equations for them. I will also be able identify spectator ions. 6. be able to choose which type of equation is most appropriate (molecular, ionic or net ionic) equation for specific situations. 7. recognize reactions which produce either CO2, H2S, or NH3 gases. 8. determine ...
... molecular and net ionic equations for them. I will also be able identify spectator ions. 6. be able to choose which type of equation is most appropriate (molecular, ionic or net ionic) equation for specific situations. 7. recognize reactions which produce either CO2, H2S, or NH3 gases. 8. determine ...
Chapter 4
... KCl(aq) + Pb(NO3)2(aq) -> 2KCl(aq) + Pb(NO3)2(aq) -> PbCl2(s) + 2KNO3(aq) AgNO3(aq) + MgBr2(aq) -> 2AgNO3(aq) + MgBr2(aq) -> 2AgBr(s) + Mg(NO3)2(aq) Ca(OH)2(aq) + FeCl3(aq) -> 3Ca(OH)2(aq) + 2FeCl3(aq) -> 2Fe(OH)3(s) + 3CaCl2(aq) NaOH(aq) + HCl(aq) -> NaOH(aq) + HCl(aq) -> H2O(l) + NaCl(aq) ...
... KCl(aq) + Pb(NO3)2(aq) -> 2KCl(aq) + Pb(NO3)2(aq) -> PbCl2(s) + 2KNO3(aq) AgNO3(aq) + MgBr2(aq) -> 2AgNO3(aq) + MgBr2(aq) -> 2AgBr(s) + Mg(NO3)2(aq) Ca(OH)2(aq) + FeCl3(aq) -> 3Ca(OH)2(aq) + 2FeCl3(aq) -> 2Fe(OH)3(s) + 3CaCl2(aq) NaOH(aq) + HCl(aq) -> NaOH(aq) + HCl(aq) -> H2O(l) + NaCl(aq) ...
Chem 150 Week 7 Handout 1 Thermochemistry (I) Define Energy
... 3 C (graphite) + 3 O2 (g) 3 CO2 (g) ...
... 3 C (graphite) + 3 O2 (g) 3 CO2 (g) ...
local section exam
... This test is designed to be taken with an answer sheet on which the student records his or her responses. All answers are to be marked on that sheet, not written in the booklet. Each student should be provided with an answer sheet and scratch paper, both of which must be turned in with the test book ...
... This test is designed to be taken with an answer sheet on which the student records his or her responses. All answers are to be marked on that sheet, not written in the booklet. Each student should be provided with an answer sheet and scratch paper, both of which must be turned in with the test book ...
Unit 12 Math and Moles
... • A chemical equation usually represents a chemical reaction. The equation will identify: • The reactants and products • The molar ratio of each of these. • Phases of matter for each substance. • Possibly some reference to energy changes in the reaction. ...
... • A chemical equation usually represents a chemical reaction. The equation will identify: • The reactants and products • The molar ratio of each of these. • Phases of matter for each substance. • Possibly some reference to energy changes in the reaction. ...
Honors Chemistry Final Review
... f. Na – OH g. Which pair of ions forms the most ionic bond: K to Cl or Fr to F? ...
... f. Na – OH g. Which pair of ions forms the most ionic bond: K to Cl or Fr to F? ...
AP Unit 0: Chemical Foundations
... Other wise they will accept answers that are ±1 sig fig. All most every question has 3 sig. fig. Therefore if you report with 3 sig fig always you’re most likely to get it correct. ...
... Other wise they will accept answers that are ±1 sig fig. All most every question has 3 sig. fig. Therefore if you report with 3 sig fig always you’re most likely to get it correct. ...
Document
... We can use Equation 3.10, relying on a periodic table to obtain the atomic weight of each component element. The atomic weights are first used to determine the formula weight of the compound. (The formula weight of C12H22O11, 342.0 amu, was calculated in Sample Exercise 3.5.) We must then do three c ...
... We can use Equation 3.10, relying on a periodic table to obtain the atomic weight of each component element. The atomic weights are first used to determine the formula weight of the compound. (The formula weight of C12H22O11, 342.0 amu, was calculated in Sample Exercise 3.5.) We must then do three c ...
Fundamentals Diagnostic Quiz
... 18. All of the following are statements from Daltons atomic hypothesis, except: a) All the atoms of a given element are identical. b) The atoms of different elements have different masses. *c) All atoms are composed of electrons, protons, and neutrons. d) A compound is a specific combination of atom ...
... 18. All of the following are statements from Daltons atomic hypothesis, except: a) All the atoms of a given element are identical. b) The atoms of different elements have different masses. *c) All atoms are composed of electrons, protons, and neutrons. d) A compound is a specific combination of atom ...
Chemical Composition
... 4. Use this as a conversion factor for moles-to-grams Molar Mass The molar mass is the mass in grams of one mole of a compound The relative weights of molecules can be calculated from atomic masses water = H2O = 2(1.008 amu) + 16.00 amu = 18.02 amu 1 mole of H2O will weigh 18.02 g, therefore ...
... 4. Use this as a conversion factor for moles-to-grams Molar Mass The molar mass is the mass in grams of one mole of a compound The relative weights of molecules can be calculated from atomic masses water = H2O = 2(1.008 amu) + 16.00 amu = 18.02 amu 1 mole of H2O will weigh 18.02 g, therefore ...
In Class Overview of Chapter
... The following increase the variety of different energy states for a given system and therefore are accompanied by an increase in entropy: 1. Increased temperature 2. Increased volume 3. Increased number of moving particles. In chemical reactions, entropy increases when: 1. gases are formed from soli ...
... The following increase the variety of different energy states for a given system and therefore are accompanied by an increase in entropy: 1. Increased temperature 2. Increased volume 3. Increased number of moving particles. In chemical reactions, entropy increases when: 1. gases are formed from soli ...
KEY_Reaction Types WS
... oxidation number (is oxidized) and another type of atom decreases in oxidation number (is reduced). A large number of oxidation-reduction (redox) reactions contain one or more reactants or products, which are pure elements. ...
... oxidation number (is oxidized) and another type of atom decreases in oxidation number (is reduced). A large number of oxidation-reduction (redox) reactions contain one or more reactants or products, which are pure elements. ...
Formulation - Good Hope School
... D. Polyvinyl chloride 26. Sodium hydroxide reacts with acids. Which of the following solutions would give the highest initial rate? A. 60 cm3 of 1.5 M NaOH(aq) and 60 cm3 of 1.5 M HCl(aq) at 30C. B. 20 cm3 of 2.0 M NaOH(aq) and 20 cm3 of 2.0 M HCl(aq) at 30C. C. 50 cm3 of 2.0 M NaOH(aq) and 50 cm3 ...
... D. Polyvinyl chloride 26. Sodium hydroxide reacts with acids. Which of the following solutions would give the highest initial rate? A. 60 cm3 of 1.5 M NaOH(aq) and 60 cm3 of 1.5 M HCl(aq) at 30C. B. 20 cm3 of 2.0 M NaOH(aq) and 20 cm3 of 2.0 M HCl(aq) at 30C. C. 50 cm3 of 2.0 M NaOH(aq) and 50 cm3 ...
LN_ch06
... The gaseous N2 so generate inflates the airbag. How many moles of NaN3 would have to decompose in order to generate 2.53 x 108 molecules of ...
... The gaseous N2 so generate inflates the airbag. How many moles of NaN3 would have to decompose in order to generate 2.53 x 108 molecules of ...
www.studyguide.pk
... Outline how stage I may be carried out to give this intermediate compound. ...
... Outline how stage I may be carried out to give this intermediate compound. ...
Advanced Placement Chemistry
... (D) Flush the affected area with water and then with a dilute NaHCO3 solution (E) Flush the affected area with water and then with a dilute vinegar solution 25. The cooling curve for a pure substance as it changes from a liquid to a solid is shown right. The solid and the liquid coexist at (A) point ...
... (D) Flush the affected area with water and then with a dilute NaHCO3 solution (E) Flush the affected area with water and then with a dilute vinegar solution 25. The cooling curve for a pure substance as it changes from a liquid to a solid is shown right. The solid and the liquid coexist at (A) point ...
Review for Physical Science Test #2
... 1. Compounds are made of ______________________ of elements that are _______________________________ together. 2. What are two ways that atoms can be bonded together? (Hint: both have to do with electrons.) ...
... 1. Compounds are made of ______________________ of elements that are _______________________________ together. 2. What are two ways that atoms can be bonded together? (Hint: both have to do with electrons.) ...
SampleTest3withAnswers
... B) 4.00 C) 0.0400 D) 3.85 _A___22. A solution is made by dissolving 15.0 mL of oil in enough gasoline to give 50.0 mL of solution. What is the % (v/v) of oil in the solution? A) 30.0 B) 23.1 C) 42.9 D) 3.33 __D__23. How many mL of 6.00 M HCl are needed to prepare 1500 mL of 0.200 M HCl solution? A) ...
... B) 4.00 C) 0.0400 D) 3.85 _A___22. A solution is made by dissolving 15.0 mL of oil in enough gasoline to give 50.0 mL of solution. What is the % (v/v) of oil in the solution? A) 30.0 B) 23.1 C) 42.9 D) 3.33 __D__23. How many mL of 6.00 M HCl are needed to prepare 1500 mL of 0.200 M HCl solution? A) ...
1C - Edexcel
... (b) Compound X is made from ethene and is used in cars to prevent the engine coolant from freezing in cold weather. (i) Compound X contains 38.7% carbon, 9.7% hydrogen and 51.6% oxygen by mass. Calculate the empirical formula of X. ...
... (b) Compound X is made from ethene and is used in cars to prevent the engine coolant from freezing in cold weather. (i) Compound X contains 38.7% carbon, 9.7% hydrogen and 51.6% oxygen by mass. Calculate the empirical formula of X. ...
Stoichiometry
Stoichiometry /ˌstɔɪkiˈɒmɨtri/ is the calculation of relative quantities of reactants and products in chemical reactions.Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers. This means that if the amounts of the separate reactants are known, then the amount of the product can be calculated. Conversely, if one reactant has a known quantity and the quantity of product can be empirically determined, then the amount of the other reactants can also be calculated.As seen in the image to the right, where the balanced equation is:CH4 + 2 O2 → CO2 + 2 H2O.Here, one molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. Stoichiometry measures these quantitative relationships, and is used to determine the amount of products/reactants that are produced/needed in a given reaction. Describing the quantitative relationships among substances as they participate in chemical reactions is known as reaction stoichiometry. In the example above, reaction stoichiometry measures the relationship between the methane and oxygen as they react to form carbon dioxide and water.Because of the well known relationship of moles to atomic weights, the ratios that are arrived at by stoichiometry can be used to determine quantities by weight in a reaction described by a balanced equation. This is called composition stoichiometry.Gas stoichiometry deals with reactions involving gases, where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases. For gases, the volume ratio is ideally the same by the ideal gas law, but the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products. In practice, due to the existence of isotopes, molar masses are used instead when calculating the mass ratio.