Unit 6: Reactions and Stoichiometry
... At the most fundamental level, the chemist needs a unit that describes a very large quantity. One of the most well-known numbers in the study of chemistry is number of units in a mole. The number of units in a mole is called Avogadro’s number (named after the Italian physicist). The mole is defined ...
... At the most fundamental level, the chemist needs a unit that describes a very large quantity. One of the most well-known numbers in the study of chemistry is number of units in a mole. The number of units in a mole is called Avogadro’s number (named after the Italian physicist). The mole is defined ...
Sec. 12.3 Day 2
... Each gas exerts a pressure proportional to its number of molecules in the container. The presence of other gas molecules does not change this fact. ...
... Each gas exerts a pressure proportional to its number of molecules in the container. The presence of other gas molecules does not change this fact. ...
1 - gcisd
... 11. When copper reacts with silver nitrate according to the equation, Cu (s) + 2 AgNO3 (aq) Cu(NO3)2 (aq) + 2 Ag (s), what is the number of grams of copper required to produce 432 grams of silver? ...
... 11. When copper reacts with silver nitrate according to the equation, Cu (s) + 2 AgNO3 (aq) Cu(NO3)2 (aq) + 2 Ag (s), what is the number of grams of copper required to produce 432 grams of silver? ...
CHEMICAL REACTIONS OBJECTIVES 1. To study reactions
... To practice balancing equations To learn solubility rules ...
... To practice balancing equations To learn solubility rules ...
Chemical Equations
... number of each type of atom on both sides of the arrow. If not, place coefficients in front of each formula to make them equal. Re-inventory each time a coefficient is added. When counting the atoms of each element, the coefficient gets distributed onto each atom in the formula it precedes. ...
... number of each type of atom on both sides of the arrow. If not, place coefficients in front of each formula to make them equal. Re-inventory each time a coefficient is added. When counting the atoms of each element, the coefficient gets distributed onto each atom in the formula it precedes. ...
B) Examples of Avagadro`s Number
... B) Make sure all formulas for reactants and products are correct, (use subscripts to balance them) and make sure all reactants are to the left of the arrow while all products are to the right of the arrow C) Count the number of atoms each element on each side to see what needs balanced Remember, unl ...
... B) Make sure all formulas for reactants and products are correct, (use subscripts to balance them) and make sure all reactants are to the left of the arrow while all products are to the right of the arrow C) Count the number of atoms each element on each side to see what needs balanced Remember, unl ...
Unit 2.2 Test Review Key
... 8.5D recognize that chemical formulas are used to identify substances and determine the number of atoms of each element in chemical formulas containing substances 8.5F recognize whether a chemical equation containing coefficients is balanced or not and how that relates to the law of conservation of ...
... 8.5D recognize that chemical formulas are used to identify substances and determine the number of atoms of each element in chemical formulas containing substances 8.5F recognize whether a chemical equation containing coefficients is balanced or not and how that relates to the law of conservation of ...
CHEMISTry is life - World of Teaching
... Precipitation reactions: When an insoluble solid called a precipitate forms when reactants are formed together. For example, when Carbon Dioxide is mixed with Calcium Hydroxide (limewater), the precipitate Calcium carbonate is formed. Ca(OH)2+CO2→H2O+Ca C03 Calcium Carbonate is found in chalk! ...
... Precipitation reactions: When an insoluble solid called a precipitate forms when reactants are formed together. For example, when Carbon Dioxide is mixed with Calcium Hydroxide (limewater), the precipitate Calcium carbonate is formed. Ca(OH)2+CO2→H2O+Ca C03 Calcium Carbonate is found in chalk! ...
SAT Practice Test 3
... b. The percent by mass of oxygen is 45% c. The percent by mass of sodium is 16% d. The percent by mass of phosphorus is 44% e. The percent by mass of hydrogen is 13% 56. Carbon and oxygen react to form carbon dioxide according to the reaction: C(s) + O2(g) → CO2(g). how much carbon dioxide can be fo ...
... b. The percent by mass of oxygen is 45% c. The percent by mass of sodium is 16% d. The percent by mass of phosphorus is 44% e. The percent by mass of hydrogen is 13% 56. Carbon and oxygen react to form carbon dioxide according to the reaction: C(s) + O2(g) → CO2(g). how much carbon dioxide can be fo ...
Le Chatelier`s Principle Quiz Answer Key
... 4. The pressure is increased. If the statement is true, write "true"on your answer sheet. If it is false, change the underlined word or words to make the statement true and write the corrected answer on your answer sheet. NH4Cl(s) + heat NH3(g) + HCl(g) 5. The above reaction is exothermic. 6. The ...
... 4. The pressure is increased. If the statement is true, write "true"on your answer sheet. If it is false, change the underlined word or words to make the statement true and write the corrected answer on your answer sheet. NH4Cl(s) + heat NH3(g) + HCl(g) 5. The above reaction is exothermic. 6. The ...
Oxidation-Reduction Reactions
... Hess’s Law Hess’s Law: When reactants are converted to products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps ...
... Hess’s Law Hess’s Law: When reactants are converted to products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps ...
Chapter 7 Chemical Reactions
... Balance the elements one at a time by using coefficients, start with elements that appear only once on each side of equation (Can not change subscripts) Odd – even principle you can make odds even, but can not make evens odd 4. Check to make sure all atoms and polyatomics are balanced 5. Make sure ...
... Balance the elements one at a time by using coefficients, start with elements that appear only once on each side of equation (Can not change subscripts) Odd – even principle you can make odds even, but can not make evens odd 4. Check to make sure all atoms and polyatomics are balanced 5. Make sure ...
AP Chemistry Review Packet 1 CO2(g) + H2(g) « H2O(g) + CO(g
... (b) Adding oxygen to the equilibrium mixture. (c) Raising the temperature of the system. ...
... (b) Adding oxygen to the equilibrium mixture. (c) Raising the temperature of the system. ...
CO 2(g) - cloudfront.net
... • In a chemical reaction, all the atoms present at the beginning are still present at the end. If all the atoms are still there, then the mass ...
... • In a chemical reaction, all the atoms present at the beginning are still present at the end. If all the atoms are still there, then the mass ...
Second Semester Extra Review
... 6. A mixture of gases is at a pressure of 920.3 mmHg, what is the partial pressure of carbon dioxide gas in the mixture containing oxygen and carbon dioxide if the partial pressure of oxygen is 524.9 mmHg? 7. What is standard temperature and pressure? 8. An oxygen gas cylinder has a volume of 5.6 x ...
... 6. A mixture of gases is at a pressure of 920.3 mmHg, what is the partial pressure of carbon dioxide gas in the mixture containing oxygen and carbon dioxide if the partial pressure of oxygen is 524.9 mmHg? 7. What is standard temperature and pressure? 8. An oxygen gas cylinder has a volume of 5.6 x ...
MOLECULAR FORMULAS N C H H C N H HHH HH
... 2. (10 points) The balanced equation for the reaction of iodine and chlorine is I2(s) + 3 Cl2(g) → 2 ICl3(g) Suppose you mix 2.0 mol of I2 with an excess of Cl2 and obtain 3.6 mol of ICl3. Complete each of the following statements: (a) The theoretical yield for ICl3 is __________ mol. (b) The actual ...
... 2. (10 points) The balanced equation for the reaction of iodine and chlorine is I2(s) + 3 Cl2(g) → 2 ICl3(g) Suppose you mix 2.0 mol of I2 with an excess of Cl2 and obtain 3.6 mol of ICl3. Complete each of the following statements: (a) The theoretical yield for ICl3 is __________ mol. (b) The actual ...
53 word equations
... Plants are able to make glucose from carbon dioxide gas in a reaction called photosynthesis. The other reactant is water, taken in through the roots. Oxygen gas is also formed in the process. Energy from the Sun is required for the reaction. ...
... Plants are able to make glucose from carbon dioxide gas in a reaction called photosynthesis. The other reactant is water, taken in through the roots. Oxygen gas is also formed in the process. Energy from the Sun is required for the reaction. ...
Periodic Table, Bonding, Reactions, and Moles
... 13. Identify the two types of bonds in the compound sodium stearate. Base your answers to questions 14 through 16 on the information below. The Solvay process is a multistep industrial process used to produce washing soda, Na2CO3 (s). In the last step of the Solvay process, NaHCO3 (s) is heated to 3 ...
... 13. Identify the two types of bonds in the compound sodium stearate. Base your answers to questions 14 through 16 on the information below. The Solvay process is a multistep industrial process used to produce washing soda, Na2CO3 (s). In the last step of the Solvay process, NaHCO3 (s) is heated to 3 ...
S.O.L. Review
... 7. Each beaker shown above contains 2.2 grams of iron and 1 liter of 3M H2SO4. Which reaction will go to completion first and why? a. Beaker A because of increased surface area. b. Beaker B because of increased surface area. c. Beaker A because of a higher concentration level. d. Beaker B because o ...
... 7. Each beaker shown above contains 2.2 grams of iron and 1 liter of 3M H2SO4. Which reaction will go to completion first and why? a. Beaker A because of increased surface area. b. Beaker B because of increased surface area. c. Beaker A because of a higher concentration level. d. Beaker B because o ...
Please use your NUMERICAL RESPONSE SHEET to answer the
... the atom is mostly empty space with a negatively charged nucleus. b. the atom is mostly empty space with a positively charged nucleus. c. the atom is very compact with a negatively charged nucleus. d. the atom is very compact with a positively charged nucleus. ...
... the atom is mostly empty space with a negatively charged nucleus. b. the atom is mostly empty space with a positively charged nucleus. c. the atom is very compact with a negatively charged nucleus. d. the atom is very compact with a positively charged nucleus. ...
3_2: More Chemical Changes
... • In today’s lab, you will be looking at chemical reactions that occur between 8 different solid materials. The solids have been dissolved in water to make solutions. ...
... • In today’s lab, you will be looking at chemical reactions that occur between 8 different solid materials. The solids have been dissolved in water to make solutions. ...
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.